Calculate the pH of a 0.050 M NH3(aq) solution.

3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of the solution at standard conditions?( HINT: What are the concentrations of all aqueous species at standard conditions?)

Calculate the pH of a mixture made by adding 54.6 mL of 0.015 M HHNO3(aq) to 142.9 mL of water at 26.6oC?

A student titrates 10.0 mL of the 2.000 M HC2H3O2(aq) with an NaOH(aq) solution of unknown concentration. The student monitors the pH during the titration. The following titration curve was created using the experimental data. Write the balanced net ionic equation for the reaction that occurs when HC2H3O2(aq) and NaOH(aq) are combined.  2.Calculate the molar concentration of the NaOH(aq) solution. 3.Explain how the student can estimate the value of Ka for HC2H3O2(aq) using the titration curve.

What is the pH of a 0.060 mol L-1 Ba(OH)2(aq) solution?

What is the pH of 3.5 × 10−4 M HNO3 (aq)?

Determine the pH of a 0.0400 mol / L solution of H 2 S (aq).

The pH of an aqueous solution of 8.39×10-2 M ammonium nitrate, NH4NO3 (aq), is

What volume, in liters, of hydrogen gas measured at STP can be produced from 50.0 mL of 6.0 M hydrobromic acid and an excess of zinc metal, according to the following reaction?

A student measures that it takes 7.21mL of 0.326 M NaOH (aq) solution to reach the first equivalence point of a titration of 100.0 mL of phosphoric acid solution. He also notes that it takes a total of 14.40 mL of 0.326 M NaOH (aq) solution to reach the second equivalence point. What is the concentration of the phosphoric acid solution?