You need to make 2.00 L of a sulfuric acid solution that has a concentration of 0.103 M. If you are going to only use 25.0 mL of stock solution to make the dilution, what must the concentration of the stock solution be?
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You need to make 2.00 L of a sulfuric acid solution that has a concentration of...
You are preparing 1.00 L of a 0.50 M solution of sulfuric acid. You have a stock bottle of concentrated acid (18 M). How much 18 M acid do you need to make your dilution in mL?
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...
Suppose you are titrating a sulfuric acid solution of unknown concentration with a sodium hydroxide solution according to the equation H2SO4 + 2NaOH + 2H2O + Na2SO4 If you require 28.52 mL of 0.904 M NaOH solution to titrate 209.1 mL of H2SO4 solution, what is the concentration of the H2SO4 solution? Type answer:
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...
You wish to make a 0.249 M hydrobromic acid solution from a stock solution of 12.0 M hydrobromic acid. How much concentrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution? __mL You wish to make a 0.112 M nitric acid solution from a stock solution of 12.0 M nitric acid. How much concentrated acid must you add to obtain a total volume of 150 mL of the dilute solution? __mL In the...
A stock solution of concentrated sulfuric acid, H2SO4, has a known concentration of 18.0M, What volume of concentrated sulfuric acid must be used to prepare 100.0ml, of 5.50M sulfuric acid solution? Select one: O a. 30.56ml O b. 0.235mL O c. 30.6ml O d. 327.3mL O e. 32.7mL
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 student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K = 1.34 x 10-6, 3.00 M O sodium bisulfate monohydrate, K = 1.20 x 10,3.00 M acetic acid, K, = 1.75 x 10-6, 5.00 M formic acid, K, = 1.77 x 10 , 2.00 M Determine which conjugate base is the best option to make a buffer at...
Sulfuric acid is generally sold as a concentrated solution that is 98.7% (by mass) sulfuric acid in water and has a density of 1.84 g/mL. What is the concentration (in M) of the commercially available concentrated sulfuric acid as described above?