How many mL of 0.116 M Ba(OH)2 are required to completely neutralize 150.0 mL of 0.280 M HNO3?

Two liters of a 1.5 M solution of sodium hydroxide are needed for a laboratory experiment. A stock solution of 5.0 M NaOH is available. How is the desired solution prepared?

3.85 The particulate drawing shown represents an aqueous so- lution of an acid HA, where A might represent an atom or group of atoms. Is HA a strong acid or a weak acid? Explain how you can tell from the picture.

Distinguish between an ionic compound and a molecular compound dissolved in water. Do all molecular compounds ionize when dissolved in water? Explain.

Explain the difference between a monoprotic acid, a diprotic acid, and a triprotic acid. Give an example of each.

Name and give the formulas of two acids that are strong electrolytes and one acid that is a weak electrolyte Name and give formulas of two bases that are strong electrolytes and one base that is a weak electrolyte.

A scientist has synthesized a diprotic organic acid, H2A, with a molar mass of 124.0 g/mol. The acid must be neutralized (forming the potassium salt) for an important experiment. Calculate the volume of 0.221 M KOH that is needed to neutralize 24.93 g of the acid, forming K2A.

Equal amounts (moles) of HCl(aq) and NaCN(aq) are mixed. The resulting solution is (a) acidic (b) basic (c) neutral

Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?

Classify the solutions represented in Exercises 9.28 and 9.30 as acidic, basic, or neutral.