How do you determine Moles, Molarity, and mass percent from titration results.

What is the molarity of the solution when 0.031 moles of NaOH are contained in 5.97 mL of solution? In the three blanks, enter the value (decimal notation with proper s.f.), units, and substance (in this order).

if 13.9ml of a solution is diluted to 94.7ml with a concentration of 0.4 M. What was the original concentration of the solution?

A chemist needs 13.46 mL of 1.17 M NaOH. What volume in mL of 3.89 M NaOH must be diluted in water to form this solution?

What volume (mL) of 0.2875 M NaOH is theoretically required to titrate 20.00 mL of 0.1276 M HCl?   What is the percent error, if the volume of 0.2875 M NaOH that is experimentally required to titrate 20.00 mL of 0.1276 M HCl is found to be 11.84 mL?

If 1.2 mL of a 7.0 M solution are diluted to 30.0 mL, what is the new concentration?

Write an equation that shows the mathematical relationship using M for molarity, L for volume in liters, and moles

Determine the molarity if 0.35 moles of NaCl was dissolved in enough water to make 200. mL of solution.

If 1.250 moles of NaCl are dissolved in a 250.0 mL solution, what is the concentration of the NaCl solution?

Calculate the new molarity if each of the following dilutions is made. Assume the volumes are additive. a) 57.2 mL of water is added to 25.5 mL of 0.129 M NaOH solution b) 108 mL of water is added to 41.9 mL of 0.658 M CaCl2 solution c) 640. mL of water is added to 106 mL of 30.1 M NaCl solution d) 349 mL of water is added to 854 mL of 1.71 M KOH solution