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pH = 4. The reason is that pH = -log [H+] or -log [H3O+] = -log 10^-4 = 4.
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∙ 7y ago
lenpollock
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A 0.00001 M solution of the strong acid HCi has pH of what?
D) 5
What is the pH of a 0.0235 M HCI solution?
- log(0.0235 M HCl)= 1.6 pH=============If I remember correctly two places are a pH designation standard.
What is the pH of a solution that contains 0.10 mole of HCI in a voulme of 100.0l?
100 Liters? I will assume as much. Molarity = moles of solute/Liters of solution Molarity = 0.10 mole HCl/100.0 Liters = 0.001 M HCl -------------------------now, to find pH - log(0.001 M HCl) = 3 pH -----------------so, your acid is of 3 pH, which is to be expected at the volume od solution
27.0 ml of 0.45 m naoh is neutralized by 20 ml of an hcl solution the molarity of the hcl solution is?
Given: 27 mL of NaOH, 0.45M; 20 mL HCI Need: M of HCI 27 ml NaOH*(1 L NaOH/1000mL NaOH)*(0.45M NaOH/1L NaOH)*(1mole HCI/1 mole NaOH)=0.012 0.012/0.02=0.607 M HCI (or rounded 0.61 M HCI)
The pH of a 0.01 M solution of HCl in water would be?
pH = - log[H+] so a 0.01 M solution of HCl has, pH= 2
A 0.00001 M solution of the strong acid HCi has pH of what?
D) 5
What is the pH of a 0.0235 M HCI solution?
- log(0.0235 M HCl)= 1.6 pH=============If I remember correctly two places are a pH designation standard.
How does the pH level of a dilute solution of HCI compare with the pH level of concentrated solution of the same acid?
A solution of HCl is highly dissociated into ions, A 0.000001 M solution (1 x 10-6) has a pH of 6 ... close to neutral. A 0.001 M solution (1 x 10-3) has a pH of 3 ... more concenterated, but still not a really concentrated solution. A 0.1 M solution (1 x 10-1) has a pH of 1 ... even more concentrated. showing it is more acidic.
What is the pH of a solution that contains 0.10 mole of HCI in a voulme of 100.0l?
100 Liters? I will assume as much. Molarity = moles of solute/Liters of solution Molarity = 0.10 mole HCl/100.0 Liters = 0.001 M HCl -------------------------now, to find pH - log(0.001 M HCl) = 3 pH -----------------so, your acid is of 3 pH, which is to be expected at the volume od solution
27.0 ml of 0.45 m naoh is neutralized by 20 ml of an hcl solution the molarity of the hcl solution is?
Given: 27 mL of NaOH, 0.45M; 20 mL HCI Need: M of HCI 27 ml NaOH*(1 L NaOH/1000mL NaOH)*(0.45M NaOH/1L NaOH)*(1mole HCI/1 mole NaOH)=0.012 0.012/0.02=0.607 M HCI (or rounded 0.61 M HCI)
The pH of a 0.01 M solution of HCl in water would be?
pH = - log[H+] so a 0.01 M solution of HCl has, pH= 2
What is the pH of a 0.001 M of HCl solution?
its PH is 3
What is the pH of a 0.5 M HF solution?
-log(0.5 M HF) = 0.3 pH
What is the pH of a .12 M solution of monochloroacetic acid?
- log(0.12 M) = 0.92 pH ---------------
What is the pH of a 0.000626 M solution of H2SO4?
- log(0.000626 M H2SO4) = 3.2 pH -----------
How would one prepare 10 ml of a 25 M HCI solution if 1 M HCI was available?
A molarity of 25? I think you have made some mistake. Please ask this question again.
What has a pH of 13.0?
A 0.01 M solution of NaOH has a pH =13
