CHM141 Concentration Practice, Exercises of Chemistry

Chm141 concentration reactions practice problems

Typology: Exercises

2025/2026

Uploaded on 12/12/2025

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CHM$141$
Professor$Jill$S.$Page$
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Molarity,$Solutions$and$Types$of$Reactions$Practice$
1. Suppose$a$solution$containing$3.50g$of$Na3PO4$is$mixed$with$a$solution$containing$6.40g$of$Ba(NO3)2.$$
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a) Write$a$balanced$molecular$equation$for$the$reaction.$
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b) Write$the$net$ionic$equation.$$Underline$the$precipitate.$
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c) How$many$grams$of$Ba3(PO4)2$can$be$formed?$
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2. To$determine$the$concentration$of$chloride$ion$in$a$100.0mL$sample$of$water,$a$chemist$adds$a$solution$of$
AgNO3$to$the$sample$to$precipitate$all$the$chlorine$ions$as$AgCl.$The$mass$of$the$precipitate$is$71.7mg.$$
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a) What$was$the$molarity$of$the$chloride$ion$in$the$original$sample$of$water?$$
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b) How$many$grams$of$chlorine$are$in$a$25mL$sample$of$the$water?$
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CHM 141

Professor Jill S. Page

Molarity, Solutions and Types of Reactions Practice

  1. Suppose a solution containing 3.50g of Na 3 PO 4 is mixed with a solution containing 6.40g of Ba(NO 3 ) 2. a) Write a balanced molecular equation for the reaction. b) Write the net ionic equation. Underline the precipitate. c) How many grams of Ba 3 (PO 4 ) 2 can be formed?
  2. To determine the concentration of chloride ion in a 100.0mL sample of water, a chemist adds a solution of AgNO 3 to the sample to precipitate all the chlorine ions as AgCl. The mass of the precipitate is 71.7mg. a) What was the molarity of the chloride ion in the original sample of water? b) How many grams of chlorine are in a 25mL sample of the water?

CHM 141

Professor Jill S. Page

  1. In an experiment, a student is asked to prepare 250.0 mL of a 0.100 M CuCl 2 solution from a stock solution of 1.75 M CuCl 2. What volume of stock solution is required to prepare this 0.100 M solution?
  2. Determine the oxidation numbers of the indicated elements in each of the following compounds: a) Oxygen in K 2 O 2 : __________ d) Chromium in Cr 2 O 7 2 - : _________ b) Mn in MnO 4 -^ : __________ e) Oxygen, O 2 : __________ c) Phosphorus in P 2 O 5 : ___________
  3. Classify each of the following redox reactions as a combination, decomposition, or displacement reaction. Write a balanced molecular equation for each, as well as total and net ionic equations for part (b), and identify the oxidizing and reducing agents in each reaction: a) magnesium ( s ) + nitrogen ( g ) → magnesium nitride ( s ) reaction type: __________________ oxidizing agent: _________________ reducing agent: _________________ b) aluminum ( s ) + lead(II) nitrate ( aq ) → aluminum nitrate ( aq ) + lead ( s ) reaction type: _____________ oxidizing agent: ___________ reducing agent: ___________