What is the pH of a 0.005 M NaOH solution?
Write a reaction equation illustrating
how water can be both an acid (according to Arhenius’ definition) and a
base (according to the Bronsted-Lowry definition).
You have to find the pH of 50 mL of an
unknown acid solution. You neutralize it by titrating it with 25
mL of a .005 M solution of NaOH. What is the pH of the unknown solution?
How many times more acidic is a solution
with a pH of 5.0 and another with a pH of 2.0? Show your work, whatever
method you decide to use.
Give an example of a neutralization reaction.
Label the reactants and the products formed.
Which of the following compounds are soluble in water?
How many grams of HBr are necessary to
make 0.5 L of 2.0 M solution?
If you add sand to water, does the boiling
point of the water become greater or less than 100oC? Explain.
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