A 25.0 mL solution of HBr is neutralized with 13.6 mL of 0.105 M Sr(OH)₂. What is the concentration of the original HBr solution?

Write a net ionic equation for any precipitation reaction that occurs when 1 M solutions of the following are mixed. (a) copper(II) sulfate and sodium chloride (b) manganese(II) nitrate and ammonium hydroxide (c) silver nitrate and hydrochloric acid (d) nickel(II) sulfate and potassium hydroxide (e) ammonium carbonate and sodium nitrate

A 8.50 g sample of KCl is dissolved in 66.0 mL of water. The resulting solution is then added to 72.0 mL of a 0.280 M CaCl2(aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution.

Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.08 11 M NaOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration of sulfuric acid in this sample of rain?

A solution of hydrochloric acid has a volume of 250. mL and a pH of 1.92. Exactly 250. mL of 0.0105 M NaOH is added. What is the pH of the resulting solution?

2. Equal amounts (moles) of acetic acid(aq) and sodium sulfite, Na2SO3(aq), are mixed. The resulting solution is acidic basic neutral

ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.

Oranges and grapefruits are known as citrus fruits because their acidity comes mainly from citric acid, H3C6H5O7. Calculate the concentration of citric acid in a solution if a 30.00-mL sample is neutralized by 15.10 mL of 0.0100 M KOH. Assume that three acidic hydrogens of each citric acid molecule are neutralized in the reaction.

A mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.

Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. Then, for each, write the net ionic equation. a NaOH + HNO3 b HCl + Ba(OH)2 c HC2H3O2 + Ca(OH)2 d NH3 + HNO3