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What is pH of h2so4?
The pH of a 0.1 M solution of sulfuric acid (H2SO4) is around 1. Note that the pH of sulfuric acid solutions will vary depending on concentration.
How will you make solution for ph4 of 0.005 normal h2so4?
To prepare a 0.005 M solution of H2SO4 with pH 4, you can first calculate the concentration of H+ ions needed to achieve a pH of 4. Then, use the dissociation of H2SO4 to determine the amount of H2SO4 needed to provide that concentration of H+ ions. Finally, dilute the calculated amount of H2SO4 with water to reach the desired volume of the solution.
What is the pH obtained on dissolving 0.01M of H2SO4 in 2 liters of solution?
The sulfuric acid (H2SO4) will dissociate into H+ and SO4^2-. Since each molecule of sulfuric acid produces 2 H+ ions, the concentration of H+ ions will be 0.02M. The pH of this solution can be calculated as pH = -log[H+], so pH = -log(0.02) ≈ 1.7.
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.
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?
To dilute the 3.5 M H2SO4 solution to 2 M, you need to add water. Use the formula M1V1 = M2V2, where M represents molarity and V represent volume. For this situation, you'll end up adding 75 ml of water to the initial 75 ml of 3.5 M H2SO4 solution to achieve a final 2 M concentration.
What is pH of h2so4?
The pH of a 0.1 M solution of sulfuric acid (H2SO4) is around 1. Note that the pH of sulfuric acid solutions will vary depending on concentration.
How will you make solution for ph4 of 0.005 normal h2so4?
To prepare a 0.005 M solution of H2SO4 with pH 4, you can first calculate the concentration of H+ ions needed to achieve a pH of 4. Then, use the dissociation of H2SO4 to determine the amount of H2SO4 needed to provide that concentration of H+ ions. Finally, dilute the calculated amount of H2SO4 with water to reach the desired volume of the solution.
What is the pH obtained on dissolving 0.01M of H2SO4 in 2 liters of solution?
The sulfuric acid (H2SO4) will dissociate into H+ and SO4^2-. Since each molecule of sulfuric acid produces 2 H+ ions, the concentration of H+ ions will be 0.02M. The pH of this solution can be calculated as pH = -log[H+], so pH = -log(0.02) ≈ 1.7.
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.
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?
To dilute the 3.5 M H2SO4 solution to 2 M, you need to add water. Use the formula M1V1 = M2V2, where M represents molarity and V represent volume. For this situation, you'll end up adding 75 ml of water to the initial 75 ml of 3.5 M H2SO4 solution to achieve a final 2 M concentration.
What is the normality of a 6.35 M H2SO4 is?
0.08 n
What volume of 6.40 m h2so4 is needed to prepare 455.0ml of a solution that is 0.700m in h2so4?
To find the volume of 6.40 M H2SO4 needed to prepare a solution that is 0.700 M, you can use the formula: M1V1 = M2V2, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume. Rearranging the formula, V1 = (M2*V2) / M1 gives you the volume: V1 = (0.700 * 455.0) / 6.40 = 49.53 ml. You would need 49.53 ml of the 6.40 M H2SO4 solution to prepare 455.0 ml of a 0.700 M H2SO4 solution.
What is the pH of a solution containing 0.1 M of HC2H3O2?
The pH of a solution containing 0.1 M of HC2H3O2 is around 2.88.
What is the pH of a 0.001 M of HCl solution?
its PH is 3
What would be the pH of a solution with a hydroxide ion OH- concentration of 10-12 M?
The pH of a solution can be calculated using the formula: pH = -log[OH-]. Therefore, for a solution with [OH-] concentration of 10-12 M, the pH would be 12.
How do you dilute a 10 M H2SO4 to 1M H2SO4?
Remember M1V1=M2V2, where M is molarity and V is volume. M1/M2=V2/V1, 10/1=v2/v1, For diluting the acid, we can add acid to water. So, assuming that 10M H2SO4 is having 1ml of water, we should add 1M of H2So4 to 10ml of water.
What is the approximate pH of a 1 M solution of Na2CO3?
The approximate pH of a 1 M solution of Na2CO3 is around 11-12, making it basic.
