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Exam 4: Types of Chemical Reactions and Solution Stoichiometry

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Question 1

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What is the net ionic equation for the reaction of aqueous sodium hydroxide with aqueous nitric acid?

A) Na⁺(aq) + OH^-(aq) + H⁺(aq) + NO₃^-(aq) → NaOH(s) + HNO₃(l)
B) H⁺(aq) + OH^-(aq) → H₂O(l)
C) Na⁺(aq) + OH^-(aq) → NaOH(s)
D) Na⁺(aq) + OH^-(aq) + H⁺(aq) + NO₃^-(aq) → Na⁺(aq) + NO₃^-(aq) + H₂O(l)
E) none of these

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Question 2

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The following reaction occurs in aqueous acid solution: NO₃^- + I^- → IO₃^- + NO₂ In the balanced equation, what is the coefficient of NO₃^-?

A) 2
B) 3
C) 4
D) 5
E) 6

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Question 3

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A 5.98-g sample consisting of a mixture of silver nitrate and sodium nitrate is dissolved in water. This aqueous mixture then reacts with aqueous barium chloride to form 3.90 g of silver chloride. Calculate the percent by mass of silver nitrate in the first mixture.

Which of the following statements is/are true of water? 1. An individual water molecule is V-shaped, with an H-O-H angle of about 105°. 2. The O-H bonds in a water molecule are ionic bonds. 3. Polar and ionic substances are more soluble in water than nonpolar substances.

Aqueous solutions of lead nitrate and potassium chloride are mixed and a precipitate forms. Which pair of ions are spectator ions?

Sulfamic acid, HSO₃NH₂ (molar mass = 97.1 g/mol) , is a strong monoprotic acid that can be used to standardize a strong base: HSO₃NH₂(aq) + KOH(aq) → KSO₂NH₂(aq) + H₂O(l) A 0) 179-g sample of HSO₃NH₂ required 19.4 mL of an aqueous solution of KOH for complete reaction. What is the molarity of the KOH solution?

Which of the following reactions does not involve oxidation-reduction?

You mix 50.0 mL of 2.00 M lead(II) nitrate with 50.0 mL of 2.00 M sodium chloride. What mass of lead(II) chloride should you form?

A 230.-mL sample of a 0.275 M solution is left on a hot plate overnight; the following morning the solution is 1.10 M. What volume of solvent has evaporated from the 0.275 M solution? (Assume volumes are additive.)

Consider five solutions that all have the same mass of solute in 100.0 mL of solution. Which has the highest concentration as measured in molarity?

1.00 mL of a 3.50 × 10^-4 M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming solution A. 2.00 mL of solution A is diluted with 8.00 mL of petroleum ether, forming solution B. How many grams of oleic acid are in 5.00 mL of solution B? (molar mass for oleic acid = 282 g/mol)

A 0.338-g sample of an unknown triprotic acid is titrated to the third equivalence point using 33.4 mL of 0.163M NaOH. Calculate the molar mass of the acid.

What volume of 0.350 M KOH is required to react completely with 24.0 mL of 0.650 M H₃PO₄?

If all of the chloride in a 5.000-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO₃, what is the percentage of chloride in the sample?

When aqueous solutions of silver nitrate and potassium chromate are mixed, the blood-red precipitate silver chromate is formed. If 10.0 mL of 0.25 M aqueous silver nitrate is mixed with 15.0 mL of 0.14 M aqueous potassium chromate, what is the total concentration of ions in the solution after the precipitate is formed?

Identify each of the following unbalanced reactions using the following choices: a) Precipitation reaction b) Acid-base reaction c) Oxidation-reduction reaction d) Combustion reaction e) More than one of answers a-d apply. -H₂SO₄ + Ba(OH)₂ → BaSO₄ + H₂O

Reacting 35.4 mL of 0.220 M AgNO₃ with 52.0 mL of 0.420 M K₂CrO₄ results in what mass of solid formed?

What is the oxidation state of chromium in K₂Cr₂O₇?

A solution contains the ions Ag⁺, Pb²⁺, and Ni²⁺. Dilute solutions of NaCl, Na₂SO₄, and Na₂S are available to separate the positive ions from each other. In order to effect separation, the solutions should be added in which order?

Write the balanced molecular equation for the reaction between aqueous solutions of lithium phosphate and sodium hydroxide.