0
Molarity is the concentration of a solution, defined as moles per unit volume.
Where,
Molarity = moles / volume
In this case the molarity of the HCl solution is 0.03 M
The pH of this is calculated by the equation below
pH = - log [H+]
Where [H+] is the concentration of hydrogen ions/ protons present in the solution.
As HCl only contains one hydrogen ion per molecule then the concentation of [H+] is 0.03 M
Then the equation can be calculated (the minus sign is very important!)
pH = - log 0.03
pH = 1.52
To summarise,
Molarity of 0.03 M HCl solution is 0.03 M
pH of 0.03 M HCl solution is 1.52
Wiki User
∙ 13y ago
Add your answer:
Earn +20 pts
What is the pH of a 0.04 M KOH solution?
0.04 M KOH produces an OH- concentration of 0.04 M. Thus, the pOH is -log 0.04 = 1.4 and the pH will be 14 - 1.4 = 12.6
What is the PH of a 1.0x10 to the negative fourth power M solution of KOH?
-log(1.0 X 10^-4 M KOH) = 4 14 - 4 = 10 pH KOH ----------------
What is the pH of a 10-5 m of koh solution?
9
What is the pH of a 1 x 10-5 M KOH solution?
9
What is the molarity of a solution with 0.2 moles of KOH in 100 mL of water?
Molarity = moles of solute/Liters of solution get moles KOH 6.31 grams KOH (1 mole KOH/56.108 grams) = 0.11246 moles KOH 0.250 M KOH = 0.11246 moles KOH/XL 0.11246/0.250 = 0.4498 liters = 450 milliliters
What is the pH of a 0.04 M KOH solution?
0.04 M KOH produces an OH- concentration of 0.04 M. Thus, the pOH is -log 0.04 = 1.4 and the pH will be 14 - 1.4 = 12.6
What is the PH of a 1.0x10 to the negative fourth power M solution of KOH?
-log(1.0 X 10^-4 M KOH) = 4 14 - 4 = 10 pH KOH ----------------
What is the pH of a 10-5 m of koh solution?
9
What is the pH of a 1 x 10-5 M KOH solution?
9
What is the pH of 3.5 x 10 -4 M solution of KOH?
-log(3.5 X 10^-4 M) = 3.4559 14 - 3.4559 = 10.5 pH
What is the molarity of a solution with 0.2 moles of KOH in 100 mL of water?
Molarity = moles of solute/Liters of solution get moles KOH 6.31 grams KOH (1 mole KOH/56.108 grams) = 0.11246 moles KOH 0.250 M KOH = 0.11246 moles KOH/XL 0.11246/0.250 = 0.4498 liters = 450 milliliters
A 30.0 ml sample of 0.200 m koh is titrated with 0.150 m hclo4 solution calculate the pH after 39.9 ml of hclo4 is added?
10.332
What is the pH of a 1.0 10-3 M KOH solution?
[OH-] = 1x10^-3 M[H+][OH-] = 1x10^-14[H+] = 1x10^-14/1x10^-3 = 1x10^-11pH = -log 1x10^-11 = 11Done another way:pOH = -log [OH-] = -log 1x10^-3 = 3pH + pOH = 14pH = 14 - 3 = 11
What volume of 0.200 m hcl is required to completely neutralize 20.00 0f 0.300 m koh?
30 mL of HCl
When KOH is added to water what does the pH of the water solution do?
The pH of water increase.
What has a pH of 13?
concentrated solution of NaOH and KOH have the pH value about 13.
What mass of KOH is needed to make 400mL of 725 M KOH?
I assume you mean 7.25 M KOH, but the process is the same anyway.Molarity = moles of solute/Liters of solution ( 400 ml = 0.4 Liters )7.25 M KOH = X moles KOH/0.4 Liters= 2.9 moles KOH (56.108 grams/1 mole KOH)= 163 grams potassium hydroxide needed===============================
