4. You have a 10.00 mL mixture of 1M sodium hydroxide and 1M sodium carbonate. You add strontium ions to precipitate out the carbonate ions and then titrate the remainder with 1.00 M HCl. The titration requires 3.33 mL of HCl. What is the percent of NaOH and Na2CO3 in the mixture?

A 25.00 mL sample of 0.1500 M lactic acid was added to a beaker. It was titrated with a 0.1700 M of NaOH in a burette. K₂ =1.4x104 of lactic acid. Calculate the pH when 8.00 mL of NaOH is added in the titration.

Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g

If 550 mL of some Pb(NO3)2 solution is mixed with 100 mL of 7.50 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M.

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

In a titration of 25.0 mL of hydrochloric acid solution with 0.107 M NaOH solution, 15.35 mL of the base are required to reach the equivalence point. What was the  molarity of the acid solution?

A solution contains 1.14×102 M magnesium nitrate and 1.13×102 M copper(II) acetate. Solid potassium hydroxide is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of hydroxide ion when this precipitation first begins? [OH]= M