Determine the concentration of NO−3 for 0.16 MM KNO3

Table 1: Titration Data Volume of magnesium hydroxide solution in Erlenmeyer flask Concentration of magnesium hydroxide 0.135 mol/L solution in Erlenmeyer flask Initial volume of nitric acid solution in burette Final volume of nitric acid solution in burette 10.Use the data in Table 1 to answer the folowing (a) Write the balanced chemical equatio. (b) Calculate the molar concentration of nitric acid 20.00 mL (c) Calculate the pH of the acid. 1.06 mL 23.08 mL

A 31.5 mL sample of a 0.489 M aqueous nitrous acid solution is titrated with a 0.425 M aqueous solution of barium hydroxide. How many milliliters of barium hydroxide must be added to reach a pH of 3.158? mL

If 15.00 mL of 3.00 M potassium iodide is needed to reach the equivalence point with 10.00 mL of lead (II) nitrate, determine the molarity of the lead (II) nitrate solution.

If 15.00 mL of 3.00 M potassium iodide is needed to reach the equivalence point with 10.00 mL of lead (II) nitrate, determine the molarity of the lead (II) nitrate solution.

A 50.0 mL solution of Mg(OH)2 of unknown concentration is titrated with 0.348 M HCI. The equivalence point (end point) is reached after 62.8 mL of HCI were dispensed into the Mg(OH)2 solution. What is the molarity concentration of the base?

A 0.396 g sample of KHPKHP will be titrated with a NaOHNaOH solution with an assumed concentration of 0.100 M. Calculate the volume of NaOH that should neutralize the KHP sample.

NiCl3NiCl3 is a strong electrolyte. Determine the concentration of each of the individual ions in a 0.650 M NiCl30.650 M NiCl3 solution.

a) What is the pH of a 0.200 Ca(OH)2 solution? b) What is the pH of a 0.200 LiOH solution? c) What is the pH of a 0.100 M HClO4 (strong acid) solution?

A 10.00 mL sample of H2SO4 acid solution requires 22.53 mL of 0.1000 M NaOH for titration. What is the molarity of the acid solution?