What is the pH of resulting solution when equal volumes of 0.1 M and H and 0.01 M HCl are mixed?

What is the pH of resulting solution when equal volumes of 0.1 M and H and 0.01 M HCl are mixed?

What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed? 12.65. 2.0.

What is the pH of 0.1 m of h2so4?

And so 0.1⋅mol⋅L−1 is 0.2⋅mol⋅L−1 with respect to H3O+ . And thus pH=−log10(0.2)=−(−0.699)=0.699 . And on the other hand, 0.1⋅N sulfuric acid is in fact 0.05⋅mol⋅L−1 with respect to sulfuric acid….the acid STILL requires TWO equivs of base for stoichiometric equivalence.

What is the pH of 0.1 M HCl and 0.1 m h2so4?

The pH of the resulting mixture is. 1.17.

How do you find the pH of a resulting solution?

Calculate the moles of the H+(aq) or OH-(aq) that is in excess. Calculate the volume of the resultant solution after the acid and base are mixed together. Calculate the concentration of the excess H+(aq) or OH-(aq) in the resultant solution. Calculate the pH of the resultant aqueous solution.

What is the pH of a 0.0125 m H2SO4 solution *?

The pH of 0.01 M sulphuric acid is 1.699.

What is the pH of the resulting solution of salt and water?

7
The pH will remain neutral at 7. Halides and alkaline metals dissociate and do not affect the H+ as the cation does not alter the H+ and the anion does not attract the H+ from water. This is why NaCl is a neutral salt.

What is the ratio of 1 mol HCl to 9 liters water?

As it is now, it would be 1 mol HCl : 1 L water, but what is needed is a ratio of 1 mol HCl : 10 L water, the latter being equivalent to 0.1 M. Therefore, to create the 0.1 M solution, you need to add 9 Liters water in relation to 1 mol HCl. If you want one liter of 0.1 M solution, take 0.1 L of the 1 M solution and pour in 0.9 L water.

What is the molarity of a solution of HCl and NaOH?

Solution is of HCL, therefore Molarity and Normality is same because n factor is one for HCl. Since, both solutions have same volume initially, so, let us take it as x. After mixing them, volume will be 2x. What is the pH of a solution by mixing 50 ml of 0.4N HCL and 50 ml 0.2 N NaOH? 10 mole of NaOH exactly neutralized by 10 mole of HCl.

What is the molar mass of H2SO4 and NaOH?

Here, the mole of H2SO4 = 20 mL x 0.1 M = 2 mmoles and the mole of NaOH = 6 mL x 0.025 M = 0.15 mmole. In this case, NaOH acts as the limiting reagent.