0
- log(0.000626 M H2SO4)
= 3.2 pH
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∙ 12y ago
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What is the pH obtained on dissolving 0.01M of H2SO4 in 2 liters of solution?
Assuming pH on just simple concentration. - log(0.01 M H2SO4) = 2 pH =====
A biochemist wishes to dilute 75 ml of an aqueous 3.5 M H2SO4 solution to an aqueous 2 M H2SO4 solution. How much water should be added to the solution?
30 mL water.
What volume of 6.40 m h2so4 is needed to prepare 455.0ml of a solution that is 0.700m in h2so4?
You need 49,8 mL H2SO4 6,4M.
What is the difference between 6 M H2SO4 and 0.1 M H2SO4?
The first solution is more concentrated because it contains 6 moles of H2SO4 per one liter of solution. The second solution is less concentrated because it contains 0.1 moles of H2SO4 in one liter. In equal amounts of each example, the first would have more H2SO4.
The pH of a 0.01 M solution of HCl in water would be?
pH = - log[H+] so a 0.01 M solution of HCl has, pH= 2
What is the pH obtained on dissolving 0.01M of H2SO4 in 2 liters of solution?
Assuming pH on just simple concentration. - log(0.01 M H2SO4) = 2 pH =====
A biochemist wishes to dilute 75 ml of an aqueous 3.5 M H2SO4 solution to an aqueous 2 M H2SO4 solution. How much water should be added to the solution?
30 mL water.
What volume of 6.40 m h2so4 is needed to prepare 455.0ml of a solution that is 0.700m in h2so4?
You need 49,8 mL H2SO4 6,4M.
What is the difference between 6 M H2SO4 and 0.1 M H2SO4?
The first solution is more concentrated because it contains 6 moles of H2SO4 per one liter of solution. The second solution is less concentrated because it contains 0.1 moles of H2SO4 in one liter. In equal amounts of each example, the first would have more H2SO4.
The pH of a 0.01 M solution of HCl in water would be?
pH = - log[H+] so a 0.01 M solution of HCl has, pH= 2
What is the pH of a 0.001 M of HCl solution?
its PH is 3
What is the normality of a 6.35 M H2SO4 is?
0.08 n
How many moles of sulfuric acid are in 500 mL of 0.324 M sulfuric acid solution?
Molarity = moles of solute/volume of solution 0.324 M H2SO4 = moles H2SO4/500 ml 162 millimoles, or, more precisely to the question 0.162 moles H2SO4
What is the pH of a 0.5 M HF solution?
-log(0.5 M HF) = 0.3 pH
What is the pH of a .12 M solution of monochloroacetic acid?
- log(0.12 M) = 0.92 pH ---------------
What has a pH of 13.0?
A 0.01 M solution of NaOH has a pH =13
What is the pH of a solution of 0.010 M HCl?
Its pH value is 2.
