11. Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag⁺ ions from 2.500 × 10² mL of a 0.0115 M AgNO₃ solution? The molar mass of NaCl is 58.44 g/mol.
____g
12. How many moles of precipitate will be formed when 45.3 mL of 0.450 M AgNO₃ is reacted with excess MgCl₂ in the following
____mol
13. If 16.5 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₃)₂, how many grams of Ni(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Ni(NO₃)₂(aq) → Ni(OH)₂ (s) + 2 NaNO₃ (aq)
____g
14. What mass of aluminum (in g) would be required to completely react with 1.95 L of 0.450 M HBr in the following chemical reaction? 2 Al(s) + 6 HBr(aq) → 2 AlBr₃ (aq) + 3 H₂(g)
____g
15. What mass of precipitate (in g) is formed when 55.2 mL of 0.500 M AlBr₃ reacts with excess AgNO₃ in the following chemical reaction? AlBr₃(aq) + 3 AgNO₃(aq) → 3 AgBr(s) + Al(NO₃)₃(aq)
____g
16. What mass of precipitate (in g) is formed when 52.2 mL of 0.500 M FeCl₃ reacts with excess AgNO₃ in the following chemical reaction? FeCl₃(aq) + 3 AgNO₃(aq) → 3 AgCl(s) + Fe(NO₃)₃(aq)
____g
17. Calculate the volume in mL of a 0.150 M NaOH solution needed to neutralize 275 mL of 0.0500 M CH₃COOH standard solution. NaOH(aq) + CH₃COOH(aq) ⇌ NaCH₃COO(aq) + H₂O(l)
_____mL
18. What volume (in mL) of 0.2750 M HBr is required to neutralize 40.00 mL of 0.8000 M NaOH?
_____mL
19. What volume (in mL) of 0.3900 M HCl is required to neutralize 75.00 mL of 0.6000 M LiOH?
_____mL
20. A 25.0 mL solution of HBr is neutralized with 23.7 mL of 0.105 M Sr(OH)₂. What is the concentration of the original HBr solution?
_____M
21. A 35.0 mL solution of Ba(OH)₂ is neutralized with 33.8 mL of 0.350 M HNO₃. What is the concentration of the original Ba(OH)₂ solution?
_____M
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