Exam 4: Reactions in Aqueous Solution

Pure acetic acid (HC₂H₃O₂)is a liquid and is known as glacial acetic acid.Calculate the molarity of a solution prepared by dissolving 20.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0 mL of solution.The density of glacial acetic acid at 25 °C is 1.05 g/mL.

Which of the following 0.300 M solutions would contain the highest concentration of potassium ions?

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 11.7 g of CH₃OH in sufficient water to give exactly 330.mL of solution?

A 0.355 M K₂SO₄ solution can be prepared by ________.

Which solution has the same number of moles of KCl as 75.00 mL of 0.250 M solution of KCl?

How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?

HNO₂ is a strong acid.

How many grams of potassium bromide are there in 250.0 mL of a 2.50 M aqueous solution of potassium bromide?

Which of the following are weak acids?

When H₂SO₄ is neutralized by NaOH in aqueous solution,the net ionic equation is ________.

Which one of the following is a weak acid?

Which compound has the atom with the highest oxidation number?

Which hydroxides are strong bases? Sr(OH)₂ KOH NaOH Ba(OH)₂

The reaction between strontium hydroxide and chloric acid produces ________.

The spectator ions in the reaction between aqueous hydrochloric acid and aqueous calcium hydroxide are ________.

Of the species below,only ________ is not an electrolyte.

Which solution contains the largest number of moles of chloride ions?

The concentration of species in 100 mL of a 3.47 M solution of sodium iodide is ________ M sodium ion and ________ M iodide ion.

A 31.5 mL aliquot of HNO₃ (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq).It took 23.9 mL of the base to reach the endpoint of the titration.The concentration (M)of the acid was ________.

________ is an oxidation reaction.