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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 volume of 0.744 Molarity of NaOH is required to titrate 10.00ml of 0.526 M H2SO4?
The balanced chemical equation for the reaction between NaOH and H2SO4 is 2NaOH + H2SO4 ⟶ Na2SO4 + 2H2O. From the equation, it is a 1:1 ratio of NaOH to H2SO4. Therefore, to neutralize 10.00 ml of 0.526 M H2SO4, you will need the same amount of 0.526 M NaOH, which is 10.00 ml.
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 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.
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.
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 volume of 0.744 Molarity of NaOH is required to titrate 10.00ml of 0.526 M H2SO4?
The balanced chemical equation for the reaction between NaOH and H2SO4 is 2NaOH + H2SO4 ⟶ Na2SO4 + 2H2O. From the equation, it is a 1:1 ratio of NaOH to H2SO4. Therefore, to neutralize 10.00 ml of 0.526 M H2SO4, you will need the same amount of 0.526 M NaOH, which is 10.00 ml.
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 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.
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 volume of 0.270 M H2SO4 is needed to react with 46.0mL of 0.100M NaOH the equation is h2so4 2naoh to na2so4 2h2oask us anything?
To find the volume of 0.270 M H2SO4 needed to react with 46.0 mL of 0.100 M NaOH, you need to use the stoichiometry of the balanced equation. The balanced equation tells you that 1 mole of H2SO4 reacts with 2 moles of NaOH. From this information, you can set up a ratio using the concentrations and volumes of the two solutions to calculate the volume of 0.270 M H2SO4 needed.
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.
How prepare 0.02 M H2So4?
To prepare a 0.02 M (molar) solution of H2SO4 (sulfuric acid), you would first need to calculate the amount of sulfuric acid needed based on its molar mass (98.08 g/mol). Then, measure out the calculated mass of H2SO4 using a balance and dissolve it in a known volume of water to make the desired concentration. For example, to make 1 liter of 0.02 M H2SO4, you would dissolve 19.62 grams of H2SO4 in enough water to make 1 liter of solution.
What is the normality of a 6.35 M H2SO4 is?
0.08 n
What is the pH of a 0.000626 M solution of H2SO4?
The pH of a 0.000626 M solution of H2SO4 would be around 3.2. This is because sulfuric acid is a strong acid and completely dissociates in water to produce two protons, resulting in an acidic solution with a low pH.
What volume of 18.0 m sulfuric acid is required to prepare 19.6 L of 0.126 m H2SO4?
Using V * M = constant at dilution = amount of H2SO4 [mol] in both of the solutionsV= volume [L] of the solutionM= molarity [mol/L] of the solutionSo: V *18.0 = 24.9 * 0.195 gives V = ( 24.9 * 0.195 ) / 18.0 = 0.270 L
What is the balanced equation of NaC3H5O3 H20 plus H2SO4 0004 M?
The balanced equation for the reaction between NaC3H5O3, H2O, and H2SO4 would be: 2NaC3H5O3 + H2SO4 + 3H2O → 2C3H6O3 + Na2SO4.
