1. How many grams for silver chromate will precipitate when 100.0 mL of 0.400 M silver nitrate solution is added to potassium chromate? 2 AgNO3(aq) K₂CRO4(04) 2 KNO3(09) + Ag₂CrO4(0) +
1. How many grams for silver chromate will precipitate when 100.0 mL of 0.400 M silver nitrate solution is added to potassium chromate? 2 AgNO3(aq) K₂CRO4(04) 2 KNO3(09) + Ag₂CrO4(0) +
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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![# Honors Chemistry Worksheet – Solution Stoichiometry
## Question 1
**How many grams of silver chromate will precipitate when 100.0 mL of 0.400 M silver nitrate solution is added to potassium chromate?**
\[ \text{2 AgNO}_3(\text{aq}) + \text{K}_2\text{CrO}_4(\text{aq}) \longrightarrow \text{2 KNO}_3(\text{aq}) + \text{Ag}_2\text{CrO}_4(\text{s}) \]
## Question 2
**If 30.0 mL of a 0.299 M sodium hydroxide solution are added to 50.0 mL of a 0.950 M cupric sulfate solution, what mass of the precipitate will form?**
\[ \text{2 NaOH}_{(\text{aq})} + \text{CuSO}_4(\text{aq}) \longrightarrow \text{Cu(OH)}_2(\text{s}) + \text{Na}_2\text{SO}_4(\text{aq}) \]
## Question 3
**What volume of 0.455 M silver nitrate solution is required to precipitate all of the bromide ions in 40.00 mL of a 0.120 M strontium bromide solution?**
\[ \text{Ag}^+_{(\text{aq})} + \text{Br}^-_{(\text{aq})} \longrightarrow \text{AgBr}_{(\text{s})} \]
## Question 4
**What volume of 2.50 M hydrobromic acid solution will be consumed in reacting with 30.00 g of aluminum metal?**
\[ \text{2 Al}_{(\text{s})} + \text{6 HBr}_{(\text{aq})} \longrightarrow \text{2 AlBr}_3(\text{aq}) + \text{3 H}_2(\text{g}) \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2b904a91-3e89-4710-bf14-7b4b1c7d4c29%2F427d8336-c07f-4423-b1f7-cd4d1ea622c2%2Fc9efueb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:# Honors Chemistry Worksheet – Solution Stoichiometry
## Question 1
**How many grams of silver chromate will precipitate when 100.0 mL of 0.400 M silver nitrate solution is added to potassium chromate?**
\[ \text{2 AgNO}_3(\text{aq}) + \text{K}_2\text{CrO}_4(\text{aq}) \longrightarrow \text{2 KNO}_3(\text{aq}) + \text{Ag}_2\text{CrO}_4(\text{s}) \]
## Question 2
**If 30.0 mL of a 0.299 M sodium hydroxide solution are added to 50.0 mL of a 0.950 M cupric sulfate solution, what mass of the precipitate will form?**
\[ \text{2 NaOH}_{(\text{aq})} + \text{CuSO}_4(\text{aq}) \longrightarrow \text{Cu(OH)}_2(\text{s}) + \text{Na}_2\text{SO}_4(\text{aq}) \]
## Question 3
**What volume of 0.455 M silver nitrate solution is required to precipitate all of the bromide ions in 40.00 mL of a 0.120 M strontium bromide solution?**
\[ \text{Ag}^+_{(\text{aq})} + \text{Br}^-_{(\text{aq})} \longrightarrow \text{AgBr}_{(\text{s})} \]
## Question 4
**What volume of 2.50 M hydrobromic acid solution will be consumed in reacting with 30.00 g of aluminum metal?**
\[ \text{2 Al}_{(\text{s})} + \text{6 HBr}_{(\text{aq})} \longrightarrow \text{2 AlBr}_3(\text{aq}) + \text{3 H}_2(\text{g}) \]
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