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Chemistry

Chemistry. Semester 2 Review. Stoichiometry. Stoichiometry. Stoichiometry. Energy. Energy. Practice Problems. Energy. Gases. Gases. Practice Problems. Acids & Bases. Gases. Acids & Bases. Practice Problems. Solutions and Concentrations. I need an in-depth explanation.

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Chemistry

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  1. Chemistry Semester 2 Review

  2. Stoichiometry Stoichiometry Stoichiometry Energy Energy Practice Problems Energy Gases Gases Practice Problems Acids & Bases Gases Acids & Bases Practice Problems Solutions and Concentrations I need an in-depth explanation I need a brief overview Practice Problems Acids & Bases I need an in-depth explanation I need a brief overview Practice Problems pH and Strength I need an in-depth explanation I need a brief overview Practice Problems

  3. Solutions, Acids, and Bases

  4. Concentrations can be measured in molarity, molality, or mole fraction • Molarity has liters solution in the denominator, while molality has kilograms solvent • The sum of mole fractions of individual substances is 1. • The process by which a substance dissolves is called solvation • A solution can be unsaturated, saturated, or supersaturated Previous Home Practice Problems Next I still don’t get it

  5. Acids dissociate in water to produce H+ ions (protons) • Bases dissociate in water to produce OH-ions • When an acid and base react, they neutralize each other, producing water and a salt. • Binary acids- add hydro-, change –ide to –ic • Oxyacids- change –ate to –ic or –ite to –ous • Strong bases are the hydroxides of the first two columns on PT, except for beryllium and magnesium • 7 Strong acids: • HCl • HI • HBr • HClO3 • HClO4 • HNO3 • H2SO4 Previous Home Practice Problems Next I still don’t get it

  6. pH = -log10[H+] = log10[H+]-1 • 10-pH = [H+] • pH of 7 is neutral, <7 is an acid, >7 is a base • Kw= [H+][OH-] = 1.00×10-14 M2 • pH + pOH = 14 • When titrating (pronounced tie-trating), convert from the molarity of the standard solution to moles, to moles of the other substance, back to molarity Previous Home Practice Problems Next I still don’t get it

  7. Solutions & Concentration

  8. A solution is a homogeneous mixture made up of a substance called a solute that is dissolved in a solvent • Solutions can be gas, liquid, or solid • If unsure, the solvent is the substance that there’s more of • An important property of a solution is its concentration • Concentration tells you how much solute there is for a given amount of solvent or solution • It can be measured in molarity, molality, or mole fraction homogeneous mixture A homogeneous mixture is uniform in composition throughout Previous Home Practice Problems Next I still don’t get it

  9. Molarity tells you how much solute there is per liter of solution. • This is the most common way of measuring concentration • The unit is 1 M= 1 mol/L (or 1M = 1000 mol/m3) Moles solute Molarity = Liters solution Previous Home Practice Problems Next I still don’t get it

  10. Molality tells you how much solute there is per kilogram of solvent. • This used with liquid solutions undergoing temperature change (because the volume and therefore molarity would change with temperature) • Used more often with solids • The unit is 1 m= 1 mol/kg Moles solute Molality = Kilograms solvent Previous Home Practice Problems Next I still don’t get it

  11. A mole fraction is just the ratio of the amount of one component to the whole solution • The sum of the mole fractions of individual components of a solution always equals one. • Unit is mol/mol or just unitless Moles A Mole Fraction Substance A = Moles A + Moles B + … Previous Home Practice Problems Next I still don’t get it

  12. When a substance dissolves in a solvent, it undergoes solvation • Solvation occurs when solvent particles surround the solute particles, and the particles of the solvent exert a greater attractive force than the one holding the solute together. O O O O O O O O Na+ Cl- H H H H H H H H H H H H H H H H Previous Home Practice Problems Next I still don’t get it

  13. The level of concentration of a solution is reflected in its saturation • A solution can be unsaturated, saturated, or supersaturated Previous Home Practice Problems Next I still don’t get it

  14. An saturated solution can’t hold any more solute without adding more solvent as well (or in other words, the concentration can’t be increased at constant temperature) • An unsaturated solution is capable of holding more solute, and its concentration can be increased until it is saturated • Saturation varies with temperature Previous Home Practice Problems Next I still don’t get it

  15. A supersaturated solution is more concentrated than a saturated solution • This is possible by raising the temperature (raising the saturation ability as well), saturating the solution, and then decreasing the temperature slowly • The solute stays dissolved, but is unstable • CO2 in soda is supersaturated, which is why it is released when soda is opened, creating fizz. Previous Home Practice Problems Next I still don’t get it

  16. Acids & Bases

  17. According to the Arrhenius model, an acid is a substance that dissociates in water to produce H+ ions (protons) • Acids often: • Have a sour taste • Sting open wounds (don’t believe me? Get a knife and some HCl) • React with most metals • Conduct electricity (because of ions) dissociates Dissociation is when an ionic compound breaks up into its compounds in an aqueous solution Previous Home Practice Problems Next I still don’t get it

  18. According to the Arrhenius model, a base is a substance that dissociates in water to produce OH- ions • Bases often: • Have a bitter taste • Feel slippery • Don’t react with most metals • Conduct electricity (because of ions) dissociates Dissociation is when an ionic compound breaks up into its compounds in an aqueous solution Previous Home Practice Problems Next I still don’t get it

  19. When an acid and a base react, they neutralize each other to produce water and a salt (& battery! No? No one?) • Both substances are neutral • *Salt can be any combination of alkali/alkaline earth metal and anion (not hydroxide) Previous Home Practice Problems Next I still don’t get it

  20. An acid-base indicator indicates whether a substance is an acid or a base • It usually does this by changing color • Litmus paper turns red in the presence of an acid, and blue in the presence of a base • Phenolphthalein is clear in an acid, and turns a base bright pink Previous Home Practice Problems Next I still don’t get it

  21. Binary acids are acids made up of hydrogen and one other element • To name a binary acid, replace the –ide ending with –ic, and add hydro- to the beginning. Add the word ‘acid’ to the end • E.g. HCl = Hydrochloric acid Previous Home Practice Problems Next I still don’t get it

  22. Oxyacids are made up of hydrogen and a polyatomic anion • To name an oxyacid, take the polyatomic ion, and if it ends with –ate, change it to –ic, and if it ends with –ite, change it to –ous. Add the word ‘acid’ to the end • An easy way to remember it is that –ate ions are used more often than –ite ions, and the –ic ending is used more often as well because of the binary acids. Previous Home Practice Problems Next I still don’t get it

  23. Strong acids and bases completely dissociate into ions when placed in water • Weak acids and bases only partially dissociate, meaning some particles form ions while others remain intact • There are seven strong acids and ten strong bases you need to memorize dissociate • HCl • HBr • HI • H2SO4 • HNO3 • HClO3 • HClO4 • LiOH • NaOH • KOH • RbOH • CsOH • FrOH • Ca(OH)2 • Sr(OH)2 • Ba(OH)2 • Ra(OH)2 Dissociation is when an ionic compound breaks up into its compounds in an aqueous solution ten strong bases seven strong acids Previous Home Practice Problems Next I still don’t get it

  24. Are you Be(OH)2? Because you’re weak and basic! (Burn!) • An easy way to remember the strong bases is that they are the hydroxides of the first two groups (alkali & alkaline earth metals) of the periodic table, excepting beryllium and magnesium (no one likes them…) Previous Home Practice Problems Next I still don’t get it

  25. Three of the seven strong acids are binary acids, and they involve the three middle elements in the halogens column (chlorine-iodine) • You can remember HClO3 and HClO4 because they both involve chlorine, and more specifically, the only two chlorine polyatomic ions to end with –ate. • Nitric and sulfuric acid both end with –ic, and involve two very common elements, nitrogen and sulfur. • Johnny was in chemistry • Johnny is no more • What he thought was H2O • Was in fact H2SO4 Previous Home Practice Problems Next I still don’t get it

  26. pH and Titrations

  27. pH stands for “power of Hydrogen” and reflects the concentration of hydrogen ions in an aqueous solution • pH is the negative decimal logarithm of the hydrogen ion concentration in a solution, or pH = -log10[H+] = log10[H+]-1 • This can be confusing because a higher pH means a lower hydrogen ion concentration (because of the negative sign) • To solve for the concentration, rearrange the equation: • pH = -log10[H+] • 10pH = 10-log[H+] • 10-pH = 10log[H+] • 10-pH = [H+] aqueous decimal logarithm An aqueous solution is one where the solvent is water • A logarithm is a function, that, when given a number and a base, will return the exponent needed to raise the base to produce that number • The decimal or common logarithm is a logarithm with a base of ten Previous Home Practice Problems Next I still don’t get it

  28. A pH of 7 is neutral • A pH < 7 is an acid (meaning the H+ concentration is greater) • A pH > 7 is a base (meaning the H+ concentration is less) Previous Home Practice Problems Next I still don’t get it

  29. The pOH reflects the hydroxide ion concentration • The product of the H+ concentration and the pH- concentration is called the equilibrium constant for that temperature • At 25˚C in water, the equilibrium constant Kw= [H+][OH-] = 1.00×10-14 M2 • Taking the logarithm of both sides: • log10([H+][OH-]) = log10(1.00×10-14) • log([H+]) + log([OH-]) = -14 • -log([H+]) - log([OH-]) = 14 • pH + pOH = 14 Previous Home Practice Problems Next I still don’t get it

  30. If you need to use more than one log/exponential when solving a problem, you’re doing it wrong. • Use the fact that [H+][OH-] = 1.00×10-14 to convert between [H+]&[OH-] without having to take logs • Use the fact that pH + pOH = 14 to find [H+] or [OH-] more quickly Previous Home Practice Problems Next I still don’t get it

  31. Titration problems can be solved by first converting the molarity of one substance (the standard solution) to moles of that substance • Convert moles of that substance to moles of the other substance • Convert moles of that substance to molarity • That’s it standard solution molarity The standard solution is the acidic or basic solution with known molarity Molarity is a measure of concentration given in moles of solute per liter of solution Previous Home Practice Problems Next I still don’t get it

  32. Still have questions? • Just email Mr. Stein! Back

  33. What is the molarity when 42g of NaOH is dissolved n 2.3L of solution? • .46M 1 H 1.00794 1 H 1.00794 2 He 2 He 3 Li 6.9 3 Li 4 Be 9.0 4 Be 5 B 5 B 6 C 6 C 12.0 7 N 7 N 14.0 8 O 16.0 8 O 9 F 9 F 19.0 10 Ne 10 Ne 11 Na 11 Na 22.99 12 Mg 12 Mg 24.3 13 Al 13 Al 14 Si 14 Si 15 P 15 P 31.0 16 S 32.1 16 S 17 Cl 17 Cl 35.5 18 Ar 18 Ar 19 K 39.1 19 K 20 Ca 20 Ca 40.1 21 Sc 21 Sc 22 Ti 22 Ti 23 V 23 V 24 Cr 24 Cr 51.996 25 Mn 25 Mn 26 Fe 26 Fe 55.845 27 Co 27 Co 28 Ni 28 Ni 29 Cu 29 Cu 30 Zn 30 Zn 31 Ga 31 Ga 32 Ge 32 Ge 33 As 33 As 34 Se 34 Se 35 Br 35 Br 36 Kr 36 Kr 37 Rb 37 Rb 38 Sr 38 Sr 39 Y 39 Y 40 Zr 40 Zr 41 Nb 41 Nb 42 Mo 42 Mo 43 Tc 43 Tc 44 Ru 44 Ru 45 Rh 45 Rh 46 Pd 46 Pd 47 Ag 47 Ag 48 Cd 48 Cd 49 In 49 In 50 Sn 50 Sn 51 Sb 51 Sb 52 Te 52 Te 53 I 53 I 54 Xe 54 Xe 55 Cs 55 Cs 56 Ba 56 Ba 57 La 57 La 72 Hf 72 Hf 73 Ta 73 Ta 74 W 74 W 75 Re 75 Re 76 Os 76 Os 77 Ir 77 Ir 78 Pt 78 Pt 79 Au 79 Au 80 Hg 80 Hg 81 Tl 81 Tl 82 Pb 82 Pb 83 Bi 83 Bi 84 Po 84 Po 85 At 85 At 86 Rn 86 Rn 87 Fr 87 Fr 88 Ra 88 Ra 89 Ac 89 Ac 104 Rf 104 Rf 105 Db 105 Db 106 Sg 106 Sg 107 Bh 107 Bh 108 Hs 108 Hs 109 Mt 109 Mt 110 Ds 110 Ds 111 Rg 111 Rg 112 Cn 112 Cn 113 Uut 113 Uut 114 Fl 114 Fl 115 Uup 115 Uup 116 Lv 116 Lv 117 Uus 117 Uus 118 Uuo 118 Uuo 58 Ce 58 Ce 59 Pr 59 Pr 60 Nd 60 Nd 61 Pm 61 Pm 62 Sm 62 Sm 63 Eu 63 Eu 64 Gd 64 Gd 65 Tb 65 Tb 66 Dy 66 Dy 67 Ho 67 Ho 68 Er 68 Er 69 Tm 69 Tm 70 Yb 70 Yb 71 Lu 71 Lu 90 Th 90 Th 91 Pa 91 Pa 92 U 92 U 93 Np 93 Np 94 Pu 94 Pu 95 Am 95 Am 96 Cm 96 Cm 97 Bk 97 Bk 98 Cf 98 Cf 99 Es 99 Es 100 Fm 100 Fm 101 Md 101 Md 102 No 102 No 103 Lr 103 Lr Previous Home Lesson Next Answer

  34. How much water should be added to 5.0g of KCl to prepare a 0.50m solution? • .13kg 1 H 1.00794 1 H 1.00794 2 He 2 He 3 Li 6.9 3 Li 4 Be 9.0 4 Be 5 B 5 B 6 C 6 C 12.0 7 N 7 N 14.0 8 O 16.0 8 O 9 F 9 F 19.0 10 Ne 10 Ne 11 Na 11 Na 22.99 12 Mg 12 Mg 24.3 13 Al 13 Al 14 Si 14 Si 15 P 15 P 31.0 16 S 32.1 16 S 17 Cl 17 Cl 35.5 18 Ar 18 Ar 19 K 39.1 19 K 20 Ca 20 Ca 40.1 21 Sc 21 Sc 22 Ti 22 Ti 23 V 23 V 24 Cr 24 Cr 51.996 25 Mn 25 Mn 26 Fe 26 Fe 55.845 27 Co 27 Co 28 Ni 28 Ni 29 Cu 29 Cu 30 Zn 30 Zn 31 Ga 31 Ga 32 Ge 32 Ge 33 As 33 As 34 Se 34 Se 35 Br 35 Br 36 Kr 36 Kr 37 Rb 37 Rb 38 Sr 38 Sr 39 Y 39 Y 40 Zr 40 Zr 41 Nb 41 Nb 42 Mo 42 Mo 43 Tc 43 Tc 44 Ru 44 Ru 45 Rh 45 Rh 46 Pd 46 Pd 47 Ag 47 Ag 48 Cd 48 Cd 49 In 49 In 50 Sn 50 Sn 51 Sb 51 Sb 52 Te 52 Te 53 I 53 I 54 Xe 54 Xe 55 Cs 55 Cs 56 Ba 56 Ba 57 La 57 La 72 Hf 72 Hf 73 Ta 73 Ta 74 W 74 W 75 Re 75 Re 76 Os 76 Os 77 Ir 77 Ir 78 Pt 78 Pt 79 Au 79 Au 80 Hg 80 Hg 81 Tl 81 Tl 82 Pb 82 Pb 83 Bi 83 Bi 84 Po 84 Po 85 At 85 At 86 Rn 86 Rn 87 Fr 87 Fr 88 Ra 88 Ra 89 Ac 89 Ac 104 Rf 104 Rf 105 Db 105 Db 106 Sg 106 Sg 107 Bh 107 Bh 108 Hs 108 Hs 109 Mt 109 Mt 110 Ds 110 Ds 111 Rg 111 Rg 112 Cn 112 Cn 113 Uut 113 Uut 114 Fl 114 Fl 115 Uup 115 Uup 116 Lv 116 Lv 117 Uus 117 Uus 118 Uuo 118 Uuo 58 Ce 58 Ce 59 Pr 59 Pr 60 Nd 60 Nd 61 Pm 61 Pm 62 Sm 62 Sm 63 Eu 63 Eu 64 Gd 64 Gd 65 Tb 65 Tb 66 Dy 66 Dy 67 Ho 67 Ho 68 Er 68 Er 69 Tm 69 Tm 70 Yb 70 Yb 71 Lu 71 Lu 90 Th 90 Th 91 Pa 91 Pa 92 U 92 U 93 Np 93 Np 94 Pu 94 Pu 95 Am 95 Am 96 Cm 96 Cm 97 Bk 97 Bk 98 Cf 98 Cf 99 Es 99 Es 100 Fm 100 Fm 101 Md 101 Md 102 No 102 No 103 Lr 103 Lr Previous Home Lesson Next Answer

  35. A gas mixture contains 70.25g of steam, 1.470g of hydrogen, and 6.58g of nitrogen. What is the mole fraction of steam? • .801 1 H 1.00794 1 H 1.00794 2 He 2 He 3 Li 3 Li 6.9 4 Be 4 Be 9.0 5 B 5 B 6 C 12.0 6 C 7 N 14.0 7 N 8 O 16.0 8 O 9 F 19.0 9 F 10 Ne 10 Ne 11 Na 22.99 11 Na 12 Mg 12 Mg 24.3 13 Al 13 Al 14 Si 14 Si 15 P 15 P 31.0 16 S 32.1 16 S 17 Cl 17 Cl 35.5 18 Ar 18 Ar 19 K 19 K 39.1 20 Ca 20 Ca 40.1 21 Sc 21 Sc 22 Ti 22 Ti 23 V 23 V 24 Cr 24 Cr 51.996 25 Mn 25 Mn 26 Fe 26 Fe 55.845 27 Co 27 Co 28 Ni 28 Ni 29 Cu 29 Cu 30 Zn 30 Zn 31 Ga 31 Ga 32 Ge 32 Ge 33 As 33 As 34 Se 34 Se 35 Br 35 Br 36 Kr 36 Kr 37 Rb 37 Rb 38 Sr 38 Sr 39 Y 39 Y 40 Zr 40 Zr 41 Nb 41 Nb 42 Mo 42 Mo 43 Tc 43 Tc 44 Ru 44 Ru 45 Rh 45 Rh 46 Pd 46 Pd 47 Ag 47 Ag 48 Cd 48 Cd 49 In 49 In 50 Sn 50 Sn 51 Sb 51 Sb 52 Te 52 Te 53 I 53 I 54 Xe 54 Xe 55 Cs 55 Cs 56 Ba 56 Ba 57 La 57 La 72 Hf 72 Hf 73 Ta 73 Ta 74 W 74 W 75 Re 75 Re 76 Os 76 Os 77 Ir 77 Ir 78 Pt 78 Pt 79 Au 79 Au 80 Hg 80 Hg 81 Tl 81 Tl 82 Pb 82 Pb 83 Bi 83 Bi 84 Po 84 Po 85 At 85 At 86 Rn 86 Rn 87 Fr 87 Fr 88 Ra 88 Ra 89 Ac 89 Ac 104 Rf 104 Rf 105 Db 105 Db 106 Sg 106 Sg 107 Bh 107 Bh 108 Hs 108 Hs 109 Mt 109 Mt 110 Ds 110 Ds 111 Rg 111 Rg 112 Cn 112 Cn 113 Uut 113 Uut 114 Fl 114 Fl 115 Uup 115 Uup 116 Lv 116 Lv 117 Uus 117 Uus 118 Uuo 118 Uuo 58 Ce 58 Ce 59 Pr 59 Pr 60 Nd 60 Nd 61 Pm 61 Pm 62 Sm 62 Sm 63 Eu 63 Eu 64 Gd 64 Gd 65 Tb 65 Tb 66 Dy 66 Dy 67 Ho 67 Ho 68 Er 68 Er 69 Tm 69 Tm 70 Yb 70 Yb 71 Lu 71 Lu 90 Th 90 Th 91 Pa 91 Pa 92 U 92 U 93 Np 93 Np 94 Pu 94 Pu 95 Am 95 Am 96 Cm 96 Cm 97 Bk 97 Bk 98 Cf 98 Cf 99 Es 99 Es 100 Fm 100 Fm 101 Md 101 Md 102 No 102 No 103 Lr 103 Lr Previous Home Lesson Next Answer

  36. What is the molality of a solid solution containing 0.125g of chromium and 1.48 moles of iron? • .0291m 1 H 1.00794 1 H 1.00794 2 He 2 He 3 Li 6.9 3 Li 4 Be 9.0 4 Be 5 B 5 B 6 C 6 C 12.0 7 N 7 N 14.0 8 O 16.0 8 O 9 F 9 F 19.0 10 Ne 10 Ne 11 Na 11 Na 22.99 12 Mg 12 Mg 24.3 13 Al 13 Al 14 Si 14 Si 15 P 15 P 31.0 16 S 32.1 16 S 17 Cl 17 Cl 35.5 18 Ar 18 Ar 19 K 39.1 19 K 20 Ca 20 Ca 40.1 21 Sc 21 Sc 22 Ti 22 Ti 23 V 23 V 24 Cr 24 Cr 51.996 25 Mn 25 Mn 26 Fe 26 Fe 55.845 27 Co 27 Co 28 Ni 28 Ni 29 Cu 29 Cu 30 Zn 30 Zn 31 Ga 31 Ga 32 Ge 32 Ge 33 As 33 As 34 Se 34 Se 35 Br 35 Br 36 Kr 36 Kr 37 Rb 37 Rb 38 Sr 38 Sr 39 Y 39 Y 40 Zr 40 Zr 41 Nb 41 Nb 42 Mo 42 Mo 43 Tc 43 Tc 44 Ru 44 Ru 45 Rh 45 Rh 46 Pd 46 Pd 47 Ag 47 Ag 48 Cd 48 Cd 49 In 49 In 50 Sn 50 Sn 51 Sb 51 Sb 52 Te 52 Te 53 I 53 I 54 Xe 54 Xe 55 Cs 55 Cs 56 Ba 56 Ba 57 La 57 La 72 Hf 72 Hf 73 Ta 73 Ta 74 W 74 W 75 Re 75 Re 76 Os 76 Os 77 Ir 77 Ir 78 Pt 78 Pt 79 Au 79 Au 80 Hg 80 Hg 81 Tl 81 Tl 82 Pb 82 Pb 83 Bi 83 Bi 84 Po 84 Po 85 At 85 At 86 Rn 86 Rn 87 Fr 87 Fr 88 Ra 88 Ra 89 Ac 89 Ac 104 Rf 104 Rf 105 Db 105 Db 106 Sg 106 Sg 107 Bh 107 Bh 108 Hs 108 Hs 109 Mt 109 Mt 110 Ds 110 Ds 111 Rg 111 Rg 112 Cn 112 Cn 113 Uut 113 Uut 114 Fl 114 Fl 115 Uup 115 Uup 116 Lv 116 Lv 117 Uus 117 Uus 118 Uuo 118 Uuo 58 Ce 58 Ce 59 Pr 59 Pr 60 Nd 60 Nd 61 Pm 61 Pm 62 Sm 62 Sm 63 Eu 63 Eu 64 Gd 64 Gd 65 Tb 65 Tb 66 Dy 66 Dy 67 Ho 67 Ho 68 Er 68 Er 69 Tm 69 Tm 70 Yb 70 Yb 71 Lu 71 Lu 90 Th 90 Th 91 Pa 91 Pa 92 U 92 U 93 Np 93 Np 94 Pu 94 Pu 95 Am 95 Am 96 Cm 96 Cm 97 Bk 97 Bk 98 Cf 98 Cf 99 Es 99 Es 100 Fm 100 Fm 101 Md 101 Md 102 No 102 No 103 Lr 103 Lr Previous Home Lesson Next Answer

  37. What is the molality of a solution in which 25g of NaCl are dissolved in 2.0kg of water? • .21m 1 H 1.00794 1 H 1.00794 2 He 2 He 3 Li 6.9 3 Li 4 Be 9.0 4 Be 5 B 5 B 6 C 6 C 12.0 7 N 7 N 14.0 8 O 16.0 8 O 9 F 9 F 19.0 10 Ne 10 Ne 11 Na 11 Na 22.99 12 Mg 12 Mg 24.3 13 Al 13 Al 14 Si 14 Si 15 P 15 P 31.0 16 S 32.1 16 S 17 Cl 17 Cl 35.5 18 Ar 18 Ar 19 K 39.1 19 K 20 Ca 20 Ca 40.1 21 Sc 21 Sc 22 Ti 22 Ti 23 V 23 V 24 Cr 24 Cr 51.996 25 Mn 25 Mn 26 Fe 26 Fe 55.845 27 Co 27 Co 28 Ni 28 Ni 29 Cu 29 Cu 30 Zn 30 Zn 31 Ga 31 Ga 32 Ge 32 Ge 33 As 33 As 34 Se 34 Se 35 Br 35 Br 36 Kr 36 Kr 37 Rb 37 Rb 38 Sr 38 Sr 39 Y 39 Y 40 Zr 40 Zr 41 Nb 41 Nb 42 Mo 42 Mo 43 Tc 43 Tc 44 Ru 44 Ru 45 Rh 45 Rh 46 Pd 46 Pd 47 Ag 47 Ag 48 Cd 48 Cd 49 In 49 In 50 Sn 50 Sn 51 Sb 51 Sb 52 Te 52 Te 53 I 53 I 54 Xe 54 Xe 55 Cs 55 Cs 56 Ba 56 Ba 57 La 57 La 72 Hf 72 Hf 73 Ta 73 Ta 74 W 74 W 75 Re 75 Re 76 Os 76 Os 77 Ir 77 Ir 78 Pt 78 Pt 79 Au 79 Au 80 Hg 80 Hg 81 Tl 81 Tl 82 Pb 82 Pb 83 Bi 83 Bi 84 Po 84 Po 85 At 85 At 86 Rn 86 Rn 87 Fr 87 Fr 88 Ra 88 Ra 89 Ac 89 Ac 104 Rf 104 Rf 105 Db 105 Db 106 Sg 106 Sg 107 Bh 107 Bh 108 Hs 108 Hs 109 Mt 109 Mt 110 Ds 110 Ds 111 Rg 111 Rg 112 Cn 112 Cn 113 Uut 113 Uut 114 Fl 114 Fl 115 Uup 115 Uup 116 Lv 116 Lv 117 Uus 117 Uus 118 Uuo 118 Uuo 58 Ce 58 Ce 59 Pr 59 Pr 60 Nd 60 Nd 61 Pm 61 Pm 62 Sm 62 Sm 63 Eu 63 Eu 64 Gd 64 Gd 65 Tb 65 Tb 66 Dy 66 Dy 67 Ho 67 Ho 68 Er 68 Er 69 Tm 69 Tm 70 Yb 70 Yb 71 Lu 71 Lu 90 Th 90 Th 91 Pa 91 Pa 92 U 92 U 93 Np 93 Np 94 Pu 94 Pu 95 Am 95 Am 96 Cm 96 Cm 97 Bk 97 Bk 98 Cf 98 Cf 99 Es 99 Es 100 Fm 100 Fm 101 Md 101 Md 102 No 102 No 103 Lr 103 Lr Previous Home Lesson Next Answer

  38. What is the molarity of the solution produced when 14.1g of ammonia (NH3) is dissolved in sufficient water to prepare .100L of solution? • 8.29 M 1 H 1.00794 1 H 1.00794 2 He 2 He 3 Li 6.9 3 Li 4 Be 9.0 4 Be 5 B 5 B 6 C 6 C 12.0 7 N 7 N 14.0 8 O 16.0 8 O 9 F 9 F 19.0 10 Ne 10 Ne 11 Na 11 Na 22.99 12 Mg 12 Mg 24.3 13 Al 13 Al 14 Si 14 Si 15 P 15 P 31.0 16 S 32.1 16 S 17 Cl 17 Cl 35.5 18 Ar 18 Ar 19 K 39.1 19 K 20 Ca 20 Ca 40.1 21 Sc 21 Sc 22 Ti 22 Ti 23 V 23 V 24 Cr 24 Cr 51.996 25 Mn 25 Mn 26 Fe 26 Fe 55.845 27 Co 27 Co 28 Ni 28 Ni 29 Cu 29 Cu 30 Zn 30 Zn 31 Ga 31 Ga 32 Ge 32 Ge 33 As 33 As 34 Se 34 Se 35 Br 35 Br 36 Kr 36 Kr 37 Rb 37 Rb 38 Sr 38 Sr 39 Y 39 Y 40 Zr 40 Zr 41 Nb 41 Nb 42 Mo 42 Mo 43 Tc 43 Tc 44 Ru 44 Ru 45 Rh 45 Rh 46 Pd 46 Pd 47 Ag 47 Ag 48 Cd 48 Cd 49 In 49 In 50 Sn 50 Sn 51 Sb 51 Sb 52 Te 52 Te 53 I 53 I 54 Xe 54 Xe 55 Cs 55 Cs 56 Ba 56 Ba 57 La 57 La 72 Hf 72 Hf 73 Ta 73 Ta 74 W 74 W 75 Re 75 Re 76 Os 76 Os 77 Ir 77 Ir 78 Pt 78 Pt 79 Au 79 Au 80 Hg 80 Hg 81 Tl 81 Tl 82 Pb 82 Pb 83 Bi 83 Bi 84 Po 84 Po 85 At 85 At 86 Rn 86 Rn 87 Fr 87 Fr 88 Ra 88 Ra 89 Ac 89 Ac 104 Rf 104 Rf 105 Db 105 Db 106 Sg 106 Sg 107 Bh 107 Bh 108 Hs 108 Hs 109 Mt 109 Mt 110 Ds 110 Ds 111 Rg 111 Rg 112 Cn 112 Cn 113 Uut 113 Uut 114 Fl 114 Fl 115 Uup 115 Uup 116 Lv 116 Lv 117 Uus 117 Uus 118 Uuo 118 Uuo 58 Ce 58 Ce 59 Pr 59 Pr 60 Nd 60 Nd 61 Pm 61 Pm 62 Sm 62 Sm 63 Eu 63 Eu 64 Gd 64 Gd 65 Tb 65 Tb 66 Dy 66 Dy 67 Ho 67 Ho 68 Er 68 Er 69 Tm 69 Tm 70 Yb 70 Yb 71 Lu 71 Lu 90 Th 90 Th 91 Pa 91 Pa 92 U 92 U 93 Np 93 Np 94 Pu 94 Pu 95 Am 95 Am 96 Cm 96 Cm 97 Bk 97 Bk 98 Cf 98 Cf 99 Es 99 Es 100 Fm 100 Fm 101 Md 101 Md 102 No 102 No 103 Lr 103 Lr Previous Home Lesson Next Answer

  39. What are some properties of acids? • Sour, sting wounds, react with metals Previous Home Lesson Next Answer

  40. Sulfuric acid • H2SO4 Previous Home Lesson Next Answer

  41. Hypochlorous acid • HClO Previous Home Lesson Next Answer

  42. H2Cr2O7 Dichromic acid Previous Home Lesson Next Answer

  43. HI • Hydroiodic acid Previous Home Lesson Next Answer

  44. What is the pH when [H+] = 9.3×10-2 M? 1.0 Previous Home Lesson Next Answer

  45. What is the pH when [OH-]= 4.30×10-3 M? 11.6 Previous Home Lesson Next Answer

  46. What is the [H+] when [OH-]= 5.8×10-7 M? 1.7×10-8M Previous Home Lesson Next Answer

  47. What is the pOH when [H+]= 1.0×10-8 M? 6 Previous Home Lesson Next Answer

  48. A volume of 50. mL of .30 M HCl neutralizes a 60. mL sample of Ca(OH)2solution. What is the concentration of Ca(OH)2? .13 M Previous Home Lesson Next Answer

  49. A volume of 20. mL of .25 M AL(OH)3 neutralizes a 75 mL sample of H2SO4 solution. What is the concentration of H2SO4? .10 M Previous Home Lesson Next Answer

  50. Incorrect Correct g 3 5 6 4 8 9 0 7 2 1 1 . 6 8 7 5 0 3 9 4 2 1 2 . 4 0 3 5 8 9 7 6 1 2 3 . 7 8 0 9 6 5 4 3 2 1 4 . 1 2 3 4 How many grams are present in 9.01 L of hydrogen gas? 1 1 1 1 1 2 2 2 2 3 3 3 3 1 2 3 4 4 4 4 5 5 5 5 6 6 6 6 2 4 5 6 7 7 7 7 8 8 8 8 9 9 9 9 3 7 8 9 . . . . 0 0 0 0 Start Over 4 Enter Enter . 0 Previous Home Lesson Next Show Answer

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