BackpH and pOH quiz #6
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1/39BackSkip to main contentBackIn what pH range is skin and hair?
Skin and hair typically have a pH of 4.5 to 6. What is the pH level of hydrogen peroxide?
Hydrogen peroxide typically has a pH around 4.5-6.5. A solution with a pH = 13 has approximately how many moles of OH– ions per liter?
pOH = 1; [OH–] = 10^-1 = 0.1 M The H+ concentration in an aqueous solution at 25°C is 5.5 x 10^-6 M. What is [OH–]?
[OH–] = Kw / [H+] = 1 x 10^-14 / 5.5 x 10^-6 ≈ 1.82 x 10^-9 M If a chemical has a pH of 3, what does this indicate?
It is strongly acidic. If the pH of beaker #1 is 2, what does this indicate?
The solution is strongly acidic. What is the [OH–] in a solution that has a [H3O+] = 1 x 10^-6 M?
[OH–] = Kw / [H3O+] = 1 x 10^-14 / 1 x 10^-6 = 1 x 10^-8 M According to the pH chart, what is the pH of pure water?
pH 7 at 25°C. Product A is 100 times more alkaline than product B. What are the most likely pHs of these products?
Product A's pH is 2 units higher than product B's. A skincare product has a pH of 2.7. What is true about this product?
It is highly acidic. If a product has a pH of 4, what does this indicate?
It is acidic. What is the average pH for hair and skin?
About 4.5 to 6. What is the pH of a 8.5 x 10^-3 M HI solution?
pH = -log(8.5 x 10^-3) ≈ 2.07 What is the pH of an 0.5 M solution of potassium bromide (KBr)?
KBr is neutral; pH ≈ 7. Which number is the most alkaline: 1, 7, 10, 14?
14. What is the pH of a 0.027 M KOH solution?
pOH = -log(0.027) ≈ 1.57; pH = 12.43 What type of graph describes the relationship between [H3O+] and pH?
An inverse logarithmic relationship. As concentration increases by a tenth, what happens to the pH?
pH decreases by 1 unit. At 25°C, aqueous solutions with a pH of 8 have a hydroxide ion concentration, [OH–], of?
pOH = 6; [OH–] = 10^-6 = 1 x 10^-6 M What happens to the H+ concentration when the pH of a solution rises by 1?
The H+ concentration decreases by a factor of 10. As concentration increases by a tenth, what happens to the pH?
pH decreases by 1 unit. Determine the pOH of a 0.00598 M HClO4 solution.
HClO4 is a strong acid; pOH = 14 - pH; pH = -log(0.00598) ≈ 2.22; pOH = 11.78 As the [H3O+] of the solution decreases, the [OH–] ________.
Increases. Determine the pH of a 0.00598 M HClO4 solution.
pH = -log(0.00598) ≈ 2.22 What is the pH of a HONH3Cl solution?
Calculate using Ka for HONH3+; solution is acidic. In a neutral solution the concentration of _____.
H+ equals OH–. A pH change can be evidence that what has occurred?
A chemical reaction or change in concentration. Rank the following solutions according to their acidity: pH 12, [H3O+] = 10^-3 M, [OH–] = 10^-7 M.
[H3O+] = 10^-3 M is most acidic, [OH–] = 10^-7 M is less acidic, pH 12 is least acidic. Calculate the pOH of this solution. Round to the nearest hundredth. pH = 1.90
pOH = 14 - 1.90 = 12.10 The hydrogen ion concentration of a solution is measured by the value.
pH. The most accurate method of measuring pH is with:
A pH meter. Vinegar has a pH of 2. Vinegar _______.
Is strongly acidic. A solution prepared by mixing 10 mL of 1 M HCl and 10 mL of 1.2 M NaOH has a pH of?
Calculate moles, find excess, determine pH. The hydrogen ion concentration of a solution is measured by the
pH value. A substance with a pH of 6 is called
Weakly acidic. What indicator would you use to know the exact pH of a substance?
A pH meter. What is the H+(aq) concentration in 0.05 M HCN(aq)? (The Ka for HCN is 5.0 x 10^-10.)
Use ICE table and Ka to solve for [H+]. What is [H+] in a 0.270 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 x 10^-5)?
Use ICE table and Ka to solve for [H+]. The pH of an acidic solution is 4.77. What is [OH–]?
pOH = 14 - 4.77 = 9.23; [OH–] = 10^-9.23 ≈ 5.89 x 10^-10 M
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