5.
We have
[OH-] = 2.52 10-9 M
We know that
pOH = -log[OH-] and pH + pOH = 14 and pH = -log[H+]
So
pOH =-log[OH-] = -log (2.52 10-9 ) = 8.59
then pH = 14 - pOH = 14 - 8.59 = 5.41
pH = 5.41
WE know that
if pH is less than 7 then solution is acidic
if pH is equal 7 then solution is neutral
if pH is more than 7 then solution is basic
here pH is 5.41 which is less than 7 so solution is Acidic
Answer = pH = 5.41 , Solution is Acidic
6.
We have
[H3O+] = 2.7 10-5 M
We know that
pH = -log[H+] = -log[H3O+]
So
pH =-log[H3O+] = -log (2.7 10-5 ) = 4.56
pH = 4.56
We know that
if pH is less than 7 then solution is acidic
if pH is equal 7 then solution is neutral
if pH is more than 7 then solution is basic
here pH is 4.56 which is less than 7 so solution is Acidic
Answer = pH = 4.56 , Solution is Acidic
7.
We have
[OH-] = 5.53 10-3 M
We know that
pOH = -log[OH-] and pH + pOH = 14
So
pOH =-log[OH-] = -log (5.53 10-3 ) = 2.25
then pH = 14 - pOH = 14 - 2.25 = 11.75
pH = 11.75
We know that
if pH is less than 7 then solution is acidic
if pH is equal 7 then solution is neutral
if pH is more than 7 then solution is basic
here pH is 11.75 which is more than 7 so solution is Basic
Answer = pH = 11.75 , Solution is Basic
5. What is the pH of a solution with a OH concentration of 2.52 x 10'M?...
QUESTION 3 What is the pH of a solution with a [OH-] concentration of 1 x 10-10 M? 02 04 08 QUESTION 4 "Is a solution with a pH of 6 acidic, basic or neutral?" O acidic basic neutral e more information needed QUESTION 5 "Is a solution with a concentration of [OH-] = 1 x 10-8 M acidic, basic, or neutral? acidic basic neutral more information needed
CHEMWORK For solutions of the same concentration, as acid strength increases [H] pH [OH-] POH Fill in the missing information in the following table. POH [H+] [OH^] Acidic, Basic or Neutral? PH Solution a 9.61 pH POH [H+] Acidic, Basic or Neutral? [OH-] M4.2 x 10-6 M Solution b pH POH [OH-] Acidic, Basic or Neutral? [H+] 0.031 M Solution pH POH 1.23 (H+] M [OH-] M Acidic, Basic or Neutral? ___ Solution d
A solution has [OH-] = 4.33 x 10-5 M. Calculate [H3O+] and pH of the solution. Then, tell whether the solution is acidic, basic, or neutral. Also, calculate pOH.
Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at 25°C. Identify the solution as acidic, basic, or neutral. Answer choice are a- 1.8 × 10^-10 M, acidic b- 1.8 × 10^-10 M, basic c- 9.2 × 10^-1 M, basic d- 9.2 × 10^-1 M, acidic e- 5.5 × 10^-10 M, neutral
Calculate the pH of a solution with OH- concentration equal to 4.3x10-9 M. Is this solution acidic, basic, or neutral?
What is the pH of a 4.0 x 10-8 M solution of HCl(aq) at 25 °C? Report your answer to the hundredths place. 6.53 0 pH = Consider the reaction. CH,CH,0 + HCECH =HCEC:" + CH, CH,OH Classify each reactant and product as an acid or base according to the Brønsted theory. Acid Base CH,CH,0 HCEC" HCECH CH,CH, OH Answer Bank Each value represents a different aqueous solution at 25°C. Classify each solution as acidic, basic, or neutral. Acidic Basic...
alculate the pH of a 0.543 M NH, solution. NH, has a Ky = 1.8 x 10 pH = Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral 0 pH = 4.59 pH=9.54 (H+) = 10x 10-7 pOH = 11.67 pOH = 4.94 (H+) - 3.7x 10-2 [H*) = 6.8 x 10- pOH = 7.00 [OH-] = 2.2 x 10- [OH-] = 5,5 x 10" Answer Bank Vhat...
Question 12 of 17 > Calculate the hydroxide ion concentration, [OH-], for a solution with a pH of 6.96. [OH-] = 3.98 x10-10 | М Incorrect Question 13 of 17 > Calculate the [OH-] and the pH of a solution with an (H+] = 6.6 x 10-12 M at 25°C. [OH-] = M pH = Calculate the (H+) and the pH of a solution with an [OH-] = 0.86 M at 25 °C. H+] = M pH = Calculate the...
9. What is the pH of a 0.125 M solution of hydrazine, N2H4? You will need to make a simplifying assumption in your calculations. (7) N2H4(aq) + H2O(l) = N2H5+(aq) + OH(aq) Kb = 1.3 x 10-6 pH: 10. What is the pH of a 2.50 M HCIO4 solution? Is this solution acidic or basic? Explain your answer. (6) pH: acidic or basic: 11. What is the conjugate base of HCO3? (3)
Fill in the missing information in the following table. [H+] [OH-] PH POH Solution a 9.63 4.37 Acidic, Basic or Neutral? Basic M pH pOH (H+ OH-1 M 4.2 x 10-6 M Acidic, Basic or Neutral? - Solution b pH POH [OH-] H+] 0.023 M Acidic, Basic or Neutral? - Solutionc M pH POH H+1 [OH-] Acidic, Basic or Neutral? - Solution d 1.27 M _ M Submit Answer Try Another Version 3 item attempts remaining