What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration .

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An analytical chemist weighs out 0.406 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 34.9 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. C mol Explanation Recheck JAHE B! F2 # 3 80 F3 X $ 4 888 F4 S % LO 5 F5 MacBook Air A 2 F6 & 7 F7 Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acc * ∞ DII F8 9 FO A F10 4 F11

2) 1.332 g primary-standard grade NazCO3 (MW = 105.99 g/mol) was used to standardize an HCI solution. Solve for the molarity of HCI if 30.19 mL of HCI was used to reach the endpoint.

Calculate the molarity of a NaOH solution if 25.85 mL of NaOH is titrated with 0.425 grams of KHP and 2.15 mL of 0.140M HCI is required.

The titration of 25.0 mL of an unknown concentration H 2SO 4 solution requires 83.6 mL of 0.12 M NaOH solution. What is the concentration of the H 2SO 4 solution (in M)?

17.65 mL of a 0.110 M sodium hydroxide solution is needed to titrate 25.00 mL of a hydrochloric acid solution to the equivalence point. a) How many moles of hydrochloric acid reacted with sodium hydroxide? b) What is the molar concentration (Molarity) of the hydrochloric acid solution?

A sodium hydroxide solution contains a small amount of sodium carbonate as a result of contamination by atmospheric carbon dioxide. A 25.00-mL aliquot requires 25.62 mL of 0.1021 M HCl to reach the phenolphthalein end point and an additional 0.80 mL to reach the methyl red end point. Calculate the molar concentration of NaOH in the solution. Type the numerical answer only.

I have a 50.0 mL sample of a solution of hydrocyanic acid, HCN, of unknown concentration. I titrate the HCN solution with a stock solution of 10.0 M NaOH. I reach endpoint when 6.50 mL of LIOH solution have been added. What is the original concentration of my HCN solution?

A 0.0250 L sample of hydrochloric acid is placed in a flask with a few drops of phenolphthalein indicator. If 0.0326 L of a 0.185 M sodium hydroxide solution is needed to reach the endpoint, what is the concentration (M) of the hydrochloric acid solution?