What is the pH of a solution that is 0.0032 M in HA and also 0.087 M in NaA? (Ka = 4.1 × 10-6) 6.56 O 4.33 6.82 8.06 5.33

Q: Calculate the [H3O+] of a 0.390 M acid solution; Ka=4.52 x10-5

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Q: A 0.045 0 M solution of HA has a pH of 2.78. Find pKa for HA.

A: Given, initial concentration of HA = 0.0450 M             pH = 2.78 We know that, pH can be…

Q: What is the pH of a 0.40 M ammonia solution? Kb = 1.85 × 10-5

A: Ammonia = 0.40 M Kb =  1.85 × 10-5 Ammonia is weak base . Kb is the dissociation constant of Ammonia…

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: A 11 mM solution of a compound with a pKa = 6.5(1L total) has a pH of 7.5.If a biochemist adds 9…

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Q: 13. What is the pH of blood with [H+] = 4.8 x 10-8 M? %3D

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Q: Find the pH of a 2.0 M solution of H2SO4. Ka = 1.1 x 10^-2

A: Given :-  Concentration of H2SO4 solution = 2.0 M  Ka of H2SO4 = 1.1 × 10-2  To find :-  pH of…

Q: What is the pH of a 0.030 M solution of KF?  Ka of HF is 7.2 x 10-4 6.19 3.16 7.81 7.60 4.67

A: The given salt is KF that is composed of KOH (strong base) and HF (weak acid). It is a basic salt.…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.100 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Ka = 4.5*10^-4 (given) pKa = – log [ Ka ] = – log(4.5*10^-4) = 3.347 Now, By using Henderson…

Q: A 0.10 M solution of a weak monoprotic acid has the solution pH = 3.10. What is the pKa for this…

A: Let us consider HA is the weak monoprotic acid. It undergoes the following dissociation reaction…

Q: 1. A1.0 M solution of a weak base B has a pH of 11.60. What is the valve of Kb for this base? а. 6.3…

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Q: What is the pH of a solution that is 0.12 M in acetic acid, HC2H3O2, and 0.50 M in sodium acetate,…

A: Given [salt] = [sodium acetate] = 0.5 M [Acid] = [Acetic Acid] = 0.12 M Ka of acetic acid = 1.8*10-5

Q: A solution is prepared from two weak acids, 0.2 M HA and 0.1 M HB. If the Ka of HA is 1x10-5 and the…

A: pH - It is the negative logarithm of the hydronium ion concentration of a  solution. Equilibrium -…

Q: Calculate the Ka of a 0.400 M acid solution with [H30*]= 1.4x 10 4M O 1.40 x 106 O 1.40 x 10 5 O…

A: Equilibrium constant is defined as products concentrations divided by reactant concentrations to the…

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

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Q: Find the pH of a 0.056 M propionic acid solution (Ka = 1.4 x 10-5). %3D

A: The reaction of propionic acid with water is written as follows:CH3CH2COOH(aq) + H2O (l)→…

Q: What is the pH of 0.41 M HCIO? Ka = 3.0 x 10-8? %3D

A: We are provided with information,  [HClO] = 0.41 M Acid dissociation constant Ka = 3.0 × 10-8  We…

Q: What is the pH of a solution when 25 ml, 0.200 M of salicylic acid CeH:(OH)COOH is diluted to 100.0…

A: Given: Concentration of salicylic acid i.e. HA (Assuming it HA as its monoprotic acid) = 0.200 M…

Q: What is the pH of an aqueous solution that is 0.011 M CH3COOH (Ka = 1.8 x 10-5) and 0.019 M…

A: An aqueous solution containing weak acid (CH3COOH) and it's conjugate base (CH3COONa) results in the…

Q: 5.796

A: Kb = 10-pKb  Kb = 10-5.796 Kb = 1.6 • 10^-6

Q: 3. What is the pH of 0.03 M acid solution? The Ka of the acid is 5x10-3? A. 1.5 В. 1.9 С. 2.0 D. 2.3

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: What is the pH of a solution that has 0.125 M CH3COOH and 0.125 M H3BO3? Ka of CH3COOH = 1.8 × 10−5…

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Q: What is the pH of a 0.0013 M solution of niacin? Ka = 1.5x10^-5

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Q: What is the pH of a solution that is 0.033 M in HA and also 0.23 Min NaA? (Kg = 4.1 × 10-6) %3D O…

A: We have to calculate the pH of solution.

Q: What is the pH of a solution that is 0.063 M in HA and also 0.023 Min NaA? (Ka = 4.1 × 10- O. 5.46…

A: Given: The concentration of HA is 0.063 M The concentration of NaA is 0.023 M The Ka value is 4.1 x…

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…

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Q: Find the pH and percent ionization of a 0.200 M HNO2 solution Ka of HNO2= 4.6 x 010-4

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Q: What is the pH of a 0.618 M carbonic acid (H2CO3) solution given Ka1=4.4×10−7 and Ka2=4.7×10−11?

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Q: What is the pH of a solution that is 0.048 M in HA and also 0.042 M in NaA? (Ka = 4.1 x 10-6) 6.82…

A: Given, Ka for NaA = 4.1 x 10-6  PH = ?

Q: 6. What is the pH of a solution containing 0.550 M HOAc and 0.460 M LiOAc? (ka of HOAc = 1.80 x…

A: The Henderson-Hasselbalch equation shows how the concentrations of an acid and its conjugate base…

Q: Calculate the pH of a solution which is 0.50 M in HA (a weak acid) and 0.80M in NaA. (Ka for HA =…

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Q: What is the pH of a 0.0520 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-10)? %3D

A: The dissociation constant(Ka) for a given reaction is defined as the ratio of concentration of…

Q: What is the pH of a 0.1055 M CH3COOH solution (Ka = 1.75 × 10−5)? 2.770…

A: Given: Ka for CH3COOH= 1.75 × 10−5 The concentration of CH3COOH, (C) =  0.1055 M.

Q: What would be the pH of a 0.12 M solution of a weak acid with Ka = 7.51 x 10^-5?    HA    <=>…

A: [HA] <===> H+ +A-   I           0.12           0       0 C            -x…

Q: What is the pH of a 0.0570 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 1010)? %3D

A: HCN is a weak acid. Hence it will dissociate partially as per the reaction HCN -----> H+ + CN-

Q: 1.58 x10-M b) Ca(OH)2 Calculate pH of 0.1 M solution of a weak base with Kb = 1.65 x10-7 %3D P=3.89

A: Weak base is taken as B.An ICE table is constructed to determine the equilibrium concentration of…

Q: Calculate the pH of a 0.01 M KCN solution, Ka for HCN = 6.2 x 10-10.   Group choices  3.40 11.8…

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Q: 3. What is the pH in a solution with [H*]=2.5x10-5? %3D

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Q: A weak acid, HA, has a pKa of 4.268. If a solution of this acid has a pH of 4.853, what percentage…

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Q: The acid dissociation constants for sulfurous acid, H2SO3, are K, = 1.7x102 and K," = 6.4x108. What…

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Q: What is the pH of a solution that is 0.12 M in acetic acid, HC2H3O2, and 0.50 M in sodium acetate,…

A: Given data [sodium acetate]=0.50 M[acetic acid]=0.12 MKa=1.8×10-5   pH of weak acid and their salt…

Q: The pH of 0.100 M Jackmanic Acid, HJa, is 2.24. What is the value of  Ka for the acid?   a. 5.4 ×…

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Q: What is the pH of 0.0050 HF (Ka = 6.8 x 10-4)?  11.27 2.30 2.73 11.70

A: The dissociation of HF can be given as follows:

Q: What is the pH of a 0.10 M weak acid with Ka = 1.8 x 10-5 ? 1.56 3.19 2.87 4.45

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Q: Find the pH and the percent hydrolysis of a 0.816 M solution of sodium o-phthalate (the salt of a…

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Q: Calculate the pH of a solution that is 0.70 M in HF (Ka =7.2 x 104) and 0.66 M in NaF. а. 3.40 O…

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Q: What is the pH of a 0.340 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The salt given is Ca(NO2)2  Since the salt is made up of strong base cation from Ca(OH)2 and anion…

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.