What is [H] in a 0.360 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 x 10 )? 1 4 7

Q: Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid…

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Q: What is the hydronium ion concentration of a 0.010 M solution of acetic acid? Ka for acetic acid is…

A: We know that : [H3O^+] = a*C ...(1)  Also, a = √(Ka/C) .....(2)  Here, Ka = 1.8*10^-5 and C = 0.010…

Q: Determine whether each of the following is true or false:(a) All strong bases are salts of the…

A: The first statement is false. Not all strong bases are salts of hydroxide ions. One of the finest…

Q: What is the pH of a solution of 8.2 x 10-5 M HCl?

A: GivenConcentration of HCl = 8.2 x 10-5 MHCl a strong electrolyte completely dissociate solutionHCl →…

Q: The value of K, at normal body temperature (37°C) is 2.8 × 10-14. Calculate the concentration of…

A: Given values : Kw = 2.8 x 10-14 [ H3O+ ] = 0.01 M

Q: acid

A: We know that acrylic acid is a weak acid therefore it will dissociate partially in the solution. The…

Q: What is [H*] in a 0.400 M solution of acrylic acid, CH;CHCOOH (Ka = 3.16 x 10-5)?

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Q: What is [H*] in a 0.240 M solution of acrylic acid, CH,CHCOOH (Ka = 3.16 x 10-5)?

A: The acid dissociation constant is the ratio of ions of the product to that of reactant when a acid…

Q: What is [H*] in a 0.250 M solution of acrylic acid, CH;CHCOOH (Ka : 3.16 x 10-5)?

A: Acrylic acid associated as - CH3CH2COOH <=> CH3CH2COO- + H+ Then by help of Following formula…

Q: What is [H⁺]

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Q: 10 10 mL 0.05 M NAOH Hd

A: Henderson's equation: pH = pKa + log[salt]/[acid] at equivalent point: [salt] = [acid] pH = pKa

Q: What is the pH of a 0.350 M triethylamine, (C2H5)3N, solution?             Kb for triethylamine is…

A: Given, 0.350 M triethylamine  Kb for triethylamine is 5.3 *10-4

Q: An aqueous solution at 25 °C has a H,0 concentration of 3.8 x 10 - 10 M. Calculate the OH…

A: The concentration of OH- is calculated as follows

Q: What is the pOH of a 0.76 M solution of citric acid, if Ka = 7.4 x 10-4 of HC6H7O7.

A: Weak acids are not completely dissociated into ions in an aqueous solution. So, when it is dissolved…

Q: A 0.55 M aqueous solution of HBRO is 4.48. What is the value of Ka for this acid? O 1.1 x 10-9 2.0 x…

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Q: Aspirin is acetylsalicylic acid, HC9H7O4, which has a Ka of 3.0 × 10-4 . Calculate the pH of a…

A: Given: Ka of acetylsalicylic acid      = 3.0 x 10-4 Mass of acetylsalicylic acid = 0.65 g Volume of…

Q: 1. Calculate the pH of the following solutions: a. 0.020M potassium acid phthalate solution; Ka =…

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Q: 25.13 mL of 0.250 M KOH is required to neutralize 10.00 mL of nitric acid. What is the concentration…

A: Volume of KOH (V1) = 25.13 mL Molarity of KOH solution (M1) = 0.250 M Volume of HNO3 solution (V2) =…

Q: 2. A 0.10 M solution of HF is 8.0% ionised. What is the K.? A. 6.4 x 104 B. 8.8 x 104 C. 6.95 x 104…

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Q: A solution of carbon dioxide in water has a hydronium ion concentration of 2.0 × 10−6 M. What is the…

A: The ionization of water takes place as,                                 2H2O(l)⇌H3O+(aq)+OH−(aq) The…

Q: The ionization constant of a very weak acid, HA, is 3.8 x 10°. Calculate the equilibrium…

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Q: What is the pH of a 0.36 M aqueous solution of the weak acid anisic acid (Ka=3.38x10^-5)?

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Q: 4. If the OH concentration in a bottle of an ammonia-based cleaner is 7.2x10° M, what is the H'…

A: (4) Ammonia based cleaner dissociates in water to give Following ions - NH3 + H2O <=> NH4+ +…

Q: 27. What is the pH of a 0.42 M solution of sodium propionate, NAC3H5O2, at 25°C? Ko(C3H5O2 ) = 7.69…

A: M

Q: What is the hydronium-ion concentration of a 0.25 M solution of HCN (Ka = 4.9 × 10–10) at 25°C?

A: Given,  Ka = 4.9×10-10 pka = -log(Ka) = -log(4.9×10-10) = 9.31 Concentration of Acid (C) = 0.25 M…

Q: What is the percent ionization of a 0.0075 M solution of ammonia? K₂(NH3) = 1.8 x 10-5 [?] % %…

A: In a solution of ammonia, ammonia is present as NH4OH due to presence of water. NH4OH acts like a…

Q: What is [H⁺] in a 0.260 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 10⁻⁵)?

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Q: A solution of 2.5 M weak acid is 1.52% ionized. What is the Ka value of this acid? cof O 32x 104 O…

A:

Q: (92) What is [OH-] in a solution of 1.25 M NH3 and 0.78 M NH4NO3? NH3 (ag) + H2 O(1) NH4 +(ag) +…

A: The reaction is given as, NH3 (aq) + H2O (l) ⇌NH4+ (aq) + OH- (aq) ; Kb = 1.8 x 10-5Kb = [NH4+]…

Q: 2. What is [OH ] in an aqueous system if the concentration of H*/H3O* is 5.0 x 10-5Ma

A: A numerical problem based on concentration of OH-, which is to be accomplished

Q: An 8.00 M solution of a weak acid, HA, is 0.47% ionized. What is the K, of the weak acid? 2.66 x…

A: Concentration of weak acid = 8.00 M  Degree of dissociation (α ) = 0.47 %  Or degree of dissociation…

Q: What are the steps to calculate pH of a 0.0532 M solution of NaCN? pKa for HCN is 9.35

A: Please find below the steps to find the pH of a 0.0532 M NaCN solution. 1) Find the concentration of…

Q: What is the pH of a solution made of 0.IM acetic acid (pka = 4.8)? %3D О а. 2.9

A: We have given that  what is pH of a solution made of 0.1M acetic acid (pKa = 4.8 )    pH of solution…

Q: A 0.050 M solution of a weak acid has [H+] = 3.8 x 10–7 M. What is the Ka for this acid?

A: Given, [H+] = 3.8 x 10–7  0.050 M solution of a weak acid

Q: What is the pH of 500.0 mL of a 0.1 M NaOH solution? O A. 13 О В. 1 ОС. 1.3 O D. 12.7 47L Ansuers to…

A: Given :  Concentration of NaOH solution  = 0.1 M

Q: A 0.10 M solution of a weak acid HA has a pH of 2.80. What is the value of Ka for HA?

A:

Q: What is the hydronium ion concentration of a 0.010 M solution of acetic acid? Ka for acetic acid is…

A: The concentration of acetic acid is equal to 0.010 M Ka for acetic acid is equal to 1.8×10-5

Q: 0.350 M KCI 6.

A: pH of 0.350M KCl is

Q: What is the [OH] of a 3.40 M solution of pyridine (C,H̟N, Kb = 1.70 × 10.9)?

A:

Q: 5. What is the approximate ratio of [A]/[HA]ions in a 0.10 M aqueous solution of H2A? Assume that…

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Q: What is the hydronium ion concentration of a 0.010 M solution of acetic acid? Ka for acetic acid is…

A:

Q: What is the pOH of an aqueous solution at 25.0 °C that contains 2.50 x 10-4 M hydronium ion?

A:

Q: 5) Find the concentration of H3O*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka=…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: 11. Calculate the pH of a .075 M orange juice solution (Ka citric acid = 1.5 x 103). %3D

A: Given, Concentration of acid, C = 0.075 M  Ionisation constant of citric acid, Ka = 1.5 × 10-3

Q: What is the pH of a solution of 0.12 M HOCl and 0.53 M NaOCl? Ka = 3.5x10-8

A: Given, Concentration of HOCl = [HOCl] = Concentration of NaOCl = [NaOCl] = Ka for HOCl = 3.5 × 10-8…

Q: In a solution with pH = 3.67, the [H] is 3.67 x 10 14 True False

A: Given data: pH = 3.67  [H+] = 3.67 x 10-14 pH = - log [H+] pH and [H+]  does not match each other.

Q: (a) Calculate the percent ionization of a 0.20 M solution of monoprotic acetylsalicylic acid…

A: (a) The H+ ion concentration is determined from given acetylsalicylic acid solution and its Ka…

Q: What is the concentration of an aqueous Ba(OH)2 that has pH = 10.3

A: Calculate OH-  concentration first then Ba(OH)2  concentration.

Q: 6) What is the hydronium ion concentration of a 0.010 M solution of acetic acid? Ka for acetic acid…

A:

Q: 1. Calculate the pH of the following solutions: a. 0.020M potassium acid phthalate solution; Ka =…

A: pH of both the solution can be found out using the equilibrium expression.