This is a set of practice problems for Solutions.
- Calculate the molarity of a solution made by dissolving 23.4 grams of sodium
sulfate in enough water to form 125 milliliters of solution. Answer
- How much 3.0 M sulfuric acid would be required to make 450 milliliters
of 0.10 M H2SO4? Answer
- How many moles of potassium ions, (K+), are present in 0.25 liters
of 0.015 M potassium carbonate? Answer
- Write balanced molecular, ionic, and net ionic equations for the precipitation
reaction (if any) that occurs when solutions of BaCl2 and Na2SO4
are mixed. Answer
- What is the molarity of an NaOH solution if 48.0 milliliters of it are needed
to neutralize 35.0 milliliters of 0.144 M H2SO4?
Answer
- What is the difference between 0.50 mol HCl and 0.50 M HCl? Answer
- Pure acetic acid, known as "glacial acetic acid," is a liquid with a density
of 1.049 g/ml at 25oC. Calculate the molarity of a solution of
acetic acid made by dissolving 10.00 milliliters of glacial acetic acid at
25oC in enough water to make 100.0 milliliters of solution. Answer
- An experiment calls for you to use 200 milliliters of 1.0 M HNO3
solution. All you have is a bottle of 6.0 M HNO3 and a tap
for distilled water. How much of the concentrated nitric acid would you need
to prepare the solution? Answer
- By titration, 15.0 milliliters of 0.1008 M NaOH is required to neutralize
a 0.2053-gram sample of an organic acid. What is the molar mass of the acid
if it contains one acidic hydrogen? An elemental analysis of the substance
indicates that it is composed of 5.89% hydrogen, 70.6% carbon, with the remainder
being oxygen. What is the molecular formula of the compound? Answer
