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Can anyone solve question 32? A basic solution does not contain H30+ A neutral solution does...
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
The following are solution concentrations. Indicate (by circling) whether each solution is acidic, basic, or neutral. Hint -- consider the power of ten in each concentration. a) 5 x 10-6 M H3O+ acidic/basic/neutral b) 5 x 10-9 M OH- acidic/basic/neutral c) 1 x 10-7 M OH- acidic/basic/neutral d) 2 x 10-3 M H3O+ acidic/basic/neutral
18) Which of the following is TRUE? 18) A) A basic solution does not contain H3O+ B) An acidic solution has [H3O+]> [OH-] C) A neutral solution contains [H20] = [H3O+] D) An neutral solution does not contain any H3O+ or OH- E) None of the above are true. 19) Determine the pH of a 0.023 M HNO3 solution. 19) A) 2.49 B) 3.68 C) 1.64 D) 12.36 E) 2.30 20) Determine the pH of a 0.188 M NH3 solution...
help! Question 5 (0.5 points) Is the following solution acidic, basic or neutral? [H30+1 = 0.95 x 10-7M. acidic basic O neutral Question 6 (0.5 points) Is the following solution acidic, basic or neutral? [H30+1 = 5.75 x 10-7M acidic basic neutral
SIMULATION Kw, Temperature, and Neutral pH 14.0 Temperature: Basic 50 °C Basic 1 → Calculate Clear 1 Neutral pH 7.01 Neutral => Neutral pH = 6.62 Kw=5.8 10-14 Acidic Acidic 0.0 0.0 50.0 Temperature (°C) 100.0 What is the [H3O+] for a neutral solution at this temperature, 50 °C? X mol/L Next (3 of 8) Recheck 5th attempt Since a neutral solution has equal concentrations of H30+ and OH-, we know that [H3O+] = [OH-] = x and Kw =...
can you please explain why the solutions say it is acidic/ basic? i dont understand the explanation one sheet. thank you. 4) What is the [H3O+] for a solution with a [OH-] of 2.73 X 102 M? Is the solution acidic, basic or neutral? *kw is constant giv The solution is basic because (OH) of 2.72 X 102 M is greater than 1.00 X 10' M. Kw = [H3O+][OH-] = 1.00 x 10-14 [H30+] = TOH-1 [OH-] = 2.72 X...
Which of the following statements describes a basic solution? 1. [H30+]> [OH] 2. [H30]<[OH] 3. [H30'] x [OH] #1 x 10-14 4. [H3O+]/[OH] = 1 x 10-14 5. [H3O+]/[OH]=1 If the pH of a solution is 10, what is the hydronium, H ion concentration? 1. A) 1 x 10-10 M 2. B) 1 x 1010 M 3. C) 10 M 4. D) 10 M 5.E) * 1 1010 M As the pH increases the hydroxide ion concentration 1. A) goes...
Instructions: Determine if each solution is acidic, basic, or neutral. [H3O+] = 1 x 10-10 M; [OH-] = 1 x 10-4 M [H3O+] = 1 x 10-7 M; [OH-] = 1 x 10-7 M [H3O+] = 1 x 10-1 M; [OH-] = 1 x 10-13 M [H3O+] = 1 x 10-13 M; [OH-] = 1 x 10-1 M Instructions: Calculate [OH-] given [H3O+] in each aqueous solution and classify the solution as acidic or basic. [H3O+] = 2.6 x 10-3...
Ignore the [OH] concentrations 62. Determine if each solution is acidic, basic, or neutral. (a) [H3O+] = 1 x 10-'M; [OH] = 1 x 10-5M. (b) [H3O+] = 1 X 10-10 M;[OH] = 1 x 10-4M (c) [H3O+] = 1 x 10-2 M;[OH-] = 1 x 10-12 M (d) [H,0*] = 1 X 10-13 M; [OH] = 1 x 10 M
1.Calculate the pH of each solution and indicate whether the solution is acidic or basic. A. [H3O+] = 1.8 x 10-4M B.[H3O-] =7.2 x 10-9M 2.Calculate the [OH-] in each solution and determine whether the solution is acidic =, basic, or neutral. A. [H3O+] = 7.5 x 10-5M B. [H3O+] = 1.5 x 10-9M C.[H3O+] = 1.0 x 10-7M 3. Write a molecular equation for the neutralization reaction between aqueous HCI and aqueous Ca(OH)2?