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18 Dec 2019

15-1) In a sample of blood at 25oC, [H3O+]= 4.6 x 10-8 M. Find the molar concentration of OH- and decide if the sample is acidic, basic, or neutral.

15-2) In a certain solution [H3O+]= 4.7 x 10-6 M. Calculate the pH and pOH of the solution.

15-3) What is the pH of a 0.04M solution of HClO4?

15-4) The pH of a solution of HNO3 was found to be 2.66. Calculate [H3O+].

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Collen Von
Collen VonLv2
31 Dec 2019

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Related questions

A solution has a pH of 5.50

(Hint: pH = – log [H3O+], that is [H3O+] = 10 – 5.50 M= 3.16 x 10–4 M ; pH + pOH = 14)

a. What is the pOH of this solution?

b. Is the solution acidic, basic, or neutral? Give reasons.

c. Calculate the concentration of [H3O+] and [OH–] in this solution

Use pH, pOH, [H3O+], and [OH–] relationships. (a) The hydroxide ion concentration in an aqueous solution of HCl is 3.4×10-13 M. Calculate [H3O+], pH, and pOH for this solution.

[H3O+] = 2.9x10^-4 M pH = 1.54 pOH = 12.46

(b) The pOH of an aqueous solution of HNO3 is 9.30. Calculate [H3O+], [OH-], and pH for this solution. [H3O+] = 2x10^-5 M [OH-] = 5x10^-10 M pH = 4.70

There is a error somewhere thank you for your help and can you give step by step aprreciate it

For each of the following salt solutions,indicate whether the solution will be acidic, basic orneutral.
Then using data given below, calculate [OH-] or[H3O+] and pH for each solution.

(a) 0.11 M NaF(Ka (HF) = 5.0 x 10-04)
1(acidic, basic, or neutral)

[OH-] = 2 M
pH = 3

(b) 0.20 MNH4Cl(Kb (NH3) = 2.0 x10-05)
4(acidic, basic, or neutral)

[H3O+] = 5 M
pH = 6

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