A 0.8159 g sample of HCl was placed into a 50 mL volumetric flask and the sample was thoroughly dissolved in water to make 50 mL of solution. It required 22.07 mL of NaOH to reach the endpoint in the titration. What is the molarity of the NaOH solution? 0.8159g Hcl

A solid acid has an equivalent mass of 92.0 g/equiv. What of this acid would require just 34.5 mL of 0.216 N NaOH for titration?

14.10 mL of 0.998 M NaOH is titrated with 0.346 M H2SO4. what volume of sulfuric acid (in mL) would be expected to fully neutralize the sodium hydroxide?

The titration demonstrated used 21.5 mL of sodium hydroxide to neutralize 25.0 mL of 1.013 M hydrochloric acid. Determine the Molarity of the sodium hydroxide solution.

A 25.00 mL sample of unknown sulfuric acid solution requires 22.62 mL of a 0.100 M NaOH to reach the equivalence point. What is the concentration of the sulfuric acid solution?

Titration of 25.0 mL of an unknown concentration H2SO4 solution requires 37.6 mL of 0.1375 M NaOH solution.  What is the concentration of the H2SO4 solution (in M)?

An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution?   2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution?   3. What is the concentration of Ag+ in solution?

A 25.2 mL sample of a 0.471 M aqueous acetic acid solution is titrated with a 0.312 M aqueous barium hydroxide solution. What is the pH at the start of the titration, before any barium hydroxide has been added? pH =

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

A 10.0 mL sample of fruit juice is titrated with 7.55mL of NaOH solution. The molar concentration of the NaOH solution of 0.101M.  A) Calculate the molar concentration of citric acid in the fruit juice. B) Determine the moles of citric acid per serving of the fruit juice. Use 240 mL as the serving size.