During the titration, 25.0 mL of the 0.0233 M saturated calcium hydroxide solution was titrated with 32.0 mL of sulfuric acid. What is the concentration of the H2SO4? Ca(OH)2 (aq) + H₂SO4 (aq) →>> CaSO4(s) + 2H₂O(1) [H₂SO4] = [?] M [H,SO ] M Enter

A technician would like to standardize an unknown Ca(OH)2 solution. It takes 18.26 mL of a 0.191 M solution of HCl to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution.  Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2. 2HCl(aq)+Ca(OH)2(aq)⟶CaCl2(aq)+2H2O(l)

Complete the equation for the dissociation of Fe(ClO4)3(aq). Omit water from the equation because it is understood to be present. Fe(ClO4)3(aq) -->

If 29.50 mL of 0.175 M nitrous acid neutralizes 50.0 mL of barium hydroxide, what is the molarity of the base ? 2HNO2 (aq) + Ba(OH)2(aq) --> Ba(NO2)2 (aq) + 2H2O (l)

A solution of hydrogen peroxide was titrated with a solution of potassium permanganate (see reaction).5 H 2O 2(aq) + 2 KMnO 4(aq) + 3 H 2SO 4 -> 5 O 2(g) + 2 MnSO 4(aq) + K 2SO 4(aq) + 8 H 2O(l)It required 75.00 mL of 0.1456 M KMnO 4 to titrate 2.623 g of the solution containing hydrogen peroxide. What was the mass percentage of H 2O 2 in the solution?

A 15.00 mL sample of barium hydroxide requires 23.55 mL of 0.2550 M hydrochloric acid to reach the titration end point. Calculate the concentration of the barium hydroxide solution. 2HCl(aq) + Ba(OH)2(aq) --> BaCl2(aq) + 2H2O(l)

55.0 mL of 1.20 M H2SO4 is added to a 39.5 mL of 2.00 M LiOH. The balanced chemical equation for the reaction is: H2SO4 (aq) + 2LiOH (aq) --> Li2SO4 (aq) + 2H2O (l)  What kind of reaction is this? If a phenolphthalein indicator was included in the reaction flask, what color will it be after the 55.0 mL of 1.20 M H2SO4 and 39.5 mL of 2.00 M LiOH have reacted? Clear or pink? Explain your answer and include any relevant calculations.

You are performing an experiment in lab that involves the titration of 25.0 mL of H2SO4 solution. You titrate the acidic solution with 0.8221 M NaOH and the equivalence point is reached by the addition of 16.25 mL of NaOH solution. Using the balanced equation below, calculate the Molarity of H2SO4 in the flask. Do NOT include units. 2NaOH(aq) + H2SO4(aq) → 2H2O(l) + Na2SO4(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 balanced chemical equation:HA(aq)+KOH(aq) --------->KA(aq)+H2O(l)       If 14.90 mL of 0.585 M KOH is required to titrate the unknown acid to the equivalence point, what is the concentration of the unknown acid? ______ M      What is the molar mass of HA? _____  g/mol

A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 20.2 mL of HNO₃ was required. How many moles of Ca(OH)2 had to be present in the initial reaction?