You have 0.765 g of an unknown acid, H₂A, which reacts with NaOH according to the balanced equation H₂A(aq) + 2 NaOH(aq) → Na2 A(aq) + 2 H₂O(l) If 25.78 mL of 0.461 M NaOH is required to titrate the acid to the second equivalence point, what is the molar mass of the acid? Molar mass = g/mol

The molarity of an aqueous solution of perchloric acid, HCIO4, is determined by titration with a 0.177 M sodium hydroxide, NaOH, solution. HCIO4 + NaOH → NaCIO4 + H20 If 25.7 mL of sodium hydroxide are required to neutralize 16.3 mL of the acid, what is the molarity of the perchloric acid solution? Molarity = M

If 16.5 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₃)₂, how many grams of Ni(OH)₂ will be formed in the following precipitation reaction?2 NaOH(aq) + Ni(NO₃)₂(aq) → Ni(OH)₂ (s) + 2 NaNO₃ (aq)

you have a 1.153 g sample of an unknown solid acid, HA, dissolved in enough water to make 20.00 mL of solution. HA reacts with KOH(aq) according to the following balances equation . HA(aq) + KOH(aq) --> KA(aq) + H2O If 12.40 mL of 0.650 M KOH is required to titrate the unknown acid to the equivalence point, what is the concentration of the unknown acid?

Consider the reaction of acetic acid (HC2H3O2) in vinegar with NaOH solution If 12.00 mL of vinegar requires 19.85 mL of 0.4500 M NaOH to reach the equivalence point. What is the molarity of the vinegar solution? (Hint, write the balanced chemical reaction.) Also, what is the mass% of acetic acid in vinegar if the density of vinegar is 1.00 g/mL?

If 28.5 g of NaOH is added to 0.750 L of 1.00 M Cd(NO₃)₂, how many grams of Cd(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Cd(NO₃)₂(aq) → Cd(OH)₂ (s) + 2 NaNO₃(aq)

Suppose you are titrating vinegar, which is an acetic acid solution of unknown concentration, with a sodium hydroxide solution according to the equation   HC2H3O2+NaOH⟶H2O+NaC2H3O2   If you require 34.58 mL of 0.1036 M NaOH solution to titrate 10.0 mL of HC2H3O2 solution, what is the molar concentration of acetic acid in the vinegar?

A 30.00-mL volume of aqueous sulfuric acid, H2SO4, is titrated using 0.200 M NaOH and an indicator that turns color only after all the sulfuric acid protons have reacted with OH- ions. The solution turns color when 48.32 mL of base has been added. What is the molar concentration of the sulfuric acid?

9. You have 0.8557 g of an unknown monoprotic acid, HA, which reacts with NaOH according to the balanced equation HA + NaOH →→ NaA + H₂O If 43.48 mL of 0.1028 M NaOH is required to titrate the acid to the equivalence point, what is the molar mass of the acid?

27.