Reference no: EM13168492
1. 0.2 M HCl is used to neutralize 20 mL of 0.35 M NaOH.
a. How many moles of OH- are present?
b. How many moles of H+ are needed to neutralize the OH-?
c. What volume of 0.2 M HCl is needed?
2. If 358 mL of H2SO4 is neutralized with 60.0 mL of 1.50 M NaOH, what is the initial concentration of the acid?
3. 78 mL of 2.5 M phosphoric acid is neutralized with 500 mL of potassium hydroxide. What is the concentration of the base?
4. When titrating 0.15 M HCl with a calcium hydroxide solution of unknown concentration, 35 mL of acid are required to neutralize 25 mL of the base.
a. Write the balanced molecular equation.
b. Write the balanced net ionic equation.
c. How many moles of H+ are present?
d. How many moles of OH- are required to neutralize the acid?
e. What is the molarity of the base?
5. A chemist dissolves 0.9 g of an unknown monoprotic (one acidic H) acid in water. She finds that 14.6 mL of 0.426 M NaOH are required to neutralize the acid.
a. How many grams of acid are present?
b. How many moles of base are required to reach the equivalence point?
c. How many moles of acid are present initially?
d. What is the molar mass of the acid?
e. What is the chemical formula and name of this acid?
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: A chemist dissolves 0.9 g of an unknown monoprotic (one acidic H) acid in water. She finds that 14.6 mL of 0.426 M NaOH are required to neutralize the acid.
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