What is the pH of 10M solution of NaOH?

this classical theory is used lot of labs. So 10M NaOH means 400gpl and it is not dilute solution. 1 M or 1 N NaOH means 40 gpl is assigned as 14 pH.

What is the pH of a 10 10M?

pH of Solution with Very Dilute Acid In this problem, a 10 – 10 M solution of HCl contributes 10 – 10 M [H +]. The ionization of water contributes 10 – 7 M [H +]. The effective [H +] of this solution is 10 – 7 M and the pH=7.

What is the pH of .00001 m NaOH?

13
You will need to know the molarity of the NaOH. Let’s assume the solution is 0.1M. NaOH is a strong base, so this will produce 0.1mol/L of OH ions in solution. This will produce a pH of 13.

How do you calculate 10M NaOH?

The molecular weight of NaOH is 40. That means you need to dissolve 40 g of NaOH in water to obtain a 1 liter of 1M (or 1N) NaOH solution. To prepare a 10M NaOH solution, you need to dissolve 10 times more NaOH i.e., 400 g of NaOH for 1 L solution.

What is the pH of a 0.10 M solution of barium hydroxide?

Therefore, the pH of a 0.10 M barium hydroxide solution is 13.3.

What is the pH of 1M NaOH?

The pH of 1M NaOH is 13 .

What is the pH of .1 M NaOH?

The pH of 1M NaOH is 13.

What is the pH of 10 7 M NaOH solution?

The pH of 10^(-7)M NaOH is 10-7MNaOH means [OH-]=10-7, pOH = 7 pH = 14 – 7 = 7.

How do you make 10 NaOH normal?

Therefore, 4 g of NaOH dissolved in one litre of solution will give N/10 NaOH solution. Weigh quickly 4 g NaOH in a beaker (as it is hygroscopic) and dissolve it in distilled water (preferably CO -free). Transfer the contents and the washings to a volumetric flask (1 litre). Cool and then make volume up to the mark.

What is the pH of a 0.10 M solution of barium hydroxide Ba OH )_( 2?

pH=−log10([H+]=5.0×10−14)=13.30 .

What is the pH of 1.2 m NaOH?

The pH of your NaOH solution is 13.