If 33.1 ml of 0.165 M hydrochloric acid requires 20.8 ml of the NaOH solution to reach the endpoint, what is the molarity of the NaOH solution?
If 33.1 ml of 0.165 M hydrochloric acid requires 20.8 ml of the NaOH solution to...
If 33.8 ml of 0.163 M hydrochloric acid requires 21.8 ml of the NaOH solution to reach the endpoint, what is the molarity of the NaOH solution?
A 25.00 mL sample of nitric acid requires 19.63 mL of 0.1103 M NaOH to reach the end point of the titration. What is the molarity of the nitric acid solution? 0.536 grams of KHP were added to 100.0mL of water. What is the molarity of the KHP solution? (Do not type units with your answer.) Following the procedure for today's lab, a 0.0206 M KHP solution requires 24.59 mL of NaOH solution to titrate it. What is the molarity...
A 0.205 M NaOH solution is used to titrate 20.0 mL of solution of H2SO4. Write a balanced equation for this acid base reaction If 45.6 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4solution. What is the PH of the solution if the hydroxide concentration [OH-] is 4.3 x 10-6M.
2. A 10.00 mL sample of aqueous H2SO, requires 20.00 mL of 0.201 M NaOH to reach the endpoint. Calculate the molarity of H2SO4
If 9.16 mL of an acetic acid solution required 9.45 mL of 1.0841 M NaOH to reach the endpoint, what's the concentration of the acetic acid solution?
If 10.24 mL of an acetic acid solution required 9.02 mL of 1.0821 M NaOH to reach the endpoint, what's the concentration of the acetic acid solution?
If 9.77 mL of an acetic Acid solution required 10.71 mL of 1.0785 M NaOH to reach the endpoint, what's the concentration of the Acetic Acid solution?
To determine the concentration of a solution of hydrochloric acid, a 75.00-mL sample is placed in a flask and titrated with a 0.1312 M solution of sodium hydroxide. A volume of 43.33 mL is required to reach the phenolphthalein endpoint. Calculate the concentration of hydrochloric acid in the original sample
A 22.55-mL sample of hydrochloric acid solution requires 20.00 mL of 0.148 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution? 1 м
An aqueous solution of hydrobromic acid is standardized by titration with a 0.165 M solution of barium hydroxide. If 19.0 mL of base are required to neutralize 22.9 mL of the acid, what is the molarity of the hydrobromic acid solution?