A 23.72 ml volume of an H 2A acid solution of unknown concentration with 2 drops...
A 23.72 ml volume of an H 2A acid solution of unknown concentration with 2 drops of phenolphthalein required 13.58 ml of 0.133 M NaOH to reach the endpoint. What is the molar concentration of the acid solution?
Homework Answers
The molarity of the H2A is 0.038M. It can
be calculated as shown
below.
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A 23.72 ml volume of an H 2A acid solution of unknown
concentration with 2 drops...
A 25.00 mL volume of an HA acid solution of unknown concentration with 2 drops of...
A 25.00 mL volume of an HA acid solution of unknown concentration with 2 drops of phenolphthalein requires 0.1320 M NaOH was put in buret to reach the endpoint in the titration. The initial reading & fina reading of NaOH is shown in the picture Initial 9.63 mL 24.16 ml Volume of HA acid (mL) Volume of NaOH (mL) Molar concentration of NaOH (molL) We were unable to transcribe this image
(4.) The flask shown here contains 0.636 g of acid and a few drops of phenolphthalein...
(4.) The flask shown here contains 0.636 g of acid and a few drops of phenolphthalein indicator dissolved in water. The buret contains 0.240 M NaOH. What volume of base is needed to reach the end point of the titration? Assuming the acid is monoprotic, what is its molar mass? (5.) 20.00 mL of a H2SO4 solution with an unknown concentration was titrated to a phenolphthalein endpoint with 39.09 mL of a 0.1315 M NaOH solution. What is the concentration...
you titrated an unknown acid with 0.0925 M NaOH, 0.6201g of the unknown acid was placed into an Erlenmeyer flask with10...
you titrated an unknown acid with 0.0925 M NaOH, 0.6201g of the unknown acid was placed into an Erlenmeyer flask with10 ml of water and 2-3 drops of phenolphthalein. It took 32.34ml of NaOH to reach the endpoint. What is the pKa of the unknown acid? pH at endpoint is 7.19.
To determine the concentration of a solution of hydrochloric acid, a 75.00-mL sample is placed in...
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
you titrated an unknown acid with 0.0925 M NaOH, 0.6201g of the unknown acid was placed...
you titrated an unknown acid with 0.0925 M NaOH, 0.6201g of the unknown acid was placed into an Erlenmeyer flask with10 ml of water and 2-3 drops of phenolphthalein. It took 32.34ml of NaOH to reach the endpoint. What is the molecular weight and the pKa of the unknown acid?
30.00 mL of an H2SO4 solution with an unknown concentration was titrated to a phenolphthalein endpoint...
30.00 mL of an H2SO4 solution with an unknown concentration was titrated to a phenolphthalein endpoint with 31.73 mL of a 0.1103 M NaOH solution. What is the concentration of the H2SO4 solution?
A 35.0 mL sample of HCl solution is placed in a flask, with a few drops...
A 35.0 mL sample of HCl solution is placed in a flask, with a few drops of phenolphthalein indicator. Of 45.9 mL of a 0.200 M solution is required to reach the endpoint, what was the concentration of the HCl solution
50.00 mL of unknown calcium hydroxide solution is titrated with 0.300 M standard nitric acid solution....
50.00 mL of unknown calcium hydroxide solution is titrated with 0.300 M standard nitric acid solution. If 42.21 mL of the standard acid so lution is required to reach a phenolphthalein endpoint, what is the molarity of the unknown calcium hydroxide solution? (Hint: write the balanced formula unit equation.)
30.00 mL of a H2SO4 Solution with an unknown concentration was titrated to a phenolphthalein endpoint with 45.43 mL of a 0.1231M NaOH solution.
30.00 mL of a H2SO4 Solution with an unknown concentration was titrated to a phenolphthalein endpoint with 45.43 mL of a 0.1231M NaOH solution.What is the concentration of the H2SO4 solution?
A 5.30 mL sample of an H3PO4 solution of unknown concentration is titrated with a 1.100×10-2...
A 5.30 mL sample of an H3PO4 solution of unknown concentration is titrated with a 1.100×10-2 M NaOH solution. A volume of 7.32 mL of the NaOH solution was required to reach the equivalence point. What is the concentration of the unknown H3PO4 solution? Express your answer with the appropriate units.
A 25.00 mL volume of an HA acid solution of unknown concentration with 2 drops of phenolphthalein requires 0.1320 M NaOH was put in buret to reach the endpoint in the titration. The initial reading & fina reading of NaOH is shown in the picture Initial 9.63 mL 24.16 ml Volume of HA acid (mL) Volume of NaOH (mL) Molar concentration of NaOH (molL) We were unable to transcribe this image
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