To determine the concentration of a solution of sulfuric acid, a 125.0-mL sample is placed in a flask and titrated with a 0.1433 M solution of cesium hydroxide. A volume of 20.29 mL is required to reach the phenolphthalein endpoint. Calculate the concentration of sulfuric acid in the original sample.
A student has 530.0 mL of a 0.1474 M aqueous solution of MnSO4 to use in an experiment. He accidentally leaves the container uncovered and comes back the next week to find only a solid residue. The mass of the residue is 18.83 g. Determine the chemical formula of this residue.
It is desired to neutralize a solution X that
contains a mixture of potassium iodide and
hydrobromic acid. Titration of
11.0 mL X with
0.147 M silver nitrate required
39.9 mL of the latter. The resulting precipitate,
containing a mixture of AgI and
AgBr, was dried and found to weigh
1.170 g. How much 0.142 M
sodium hydroxide should be used to neutralize
11.0 mL solution X?
To determine the concentration of a solution of sulfuric acid, a 125.0-mL sample is placed in...
11. To determine the concentration of a solution of sulfuric acid, a chemist titrates the solution with aqueous potassium hydroxide. She finds that 21.4 mL of 2.50 M aq. KOH is required to neutralize 10.0 mL of aq, HSO a. Write the balanced equation for this neutralization reaction b. What was the concentration of the H2SO4 solution?
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1435 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 13.55 mL of the standard solution. What...
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1494 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 18.48 mL of the standard solution. What...
It is desired to neutralize a solution X that contains a mixture of potassium iodide and hydrobromic acid. Titration of 10.2 mL X with 0.113 M silver nitrate required 62.5 mL of the latter. The resulting precipitate, containing a mixture of AgI and AgBr, was dried and found to weigh 1.410 g. How much 0.147 M sodium hydroxide should be used to neutralize 10.2 mL solution X?
A 25.00 mL sample of an unknown sulfuric acid solution is titrated with 29.84 mL of a sodium hydroxide solution with a concentration of 0.150 M NaOH. What is the concentration of the sulfuric acid solution? H.SO.(aq) + 2NaOH(aq) → Na2SO4 (aq) + 2 H2O(1) Show your work Final Answer
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 are asked to tittate a sample of sulfuric acid of unknown concentration against a standardized solution if sodium hydroxide. you stsrt with 23.00 mL of sulfuric acid in a reaction flask, and 25.67 mL of 1.760 M sodium hydroxide are required to reach the equivalent point, what is the molarity (M) of the sulfuric acid solution? please show conversion steps!
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1659 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 11.76 mL of the standard solution. What...
94.20 mL of 0.800 M potassium hydroxide reacts with 125.0 mL of a solution containing oxalic acid, H2C2O4, which is a diprotic species. What is the concentration of the acid solution?
In a titration, 37.47 mL of a 0.2088 M solution of potassium hydroxide were required to neutralize 25.00 mL of sulfuric acid. What is the concentration of the sulfuric acid solution?