What is the pH for 1.4 M CH3COONa aqueous solution (CH3COOH, Ka=1.8×10-5)?

Q: What volume of (0.45 M) Ca(OH)2 must be added to 50 mL of 0.25-M (KOH) to give a solution 0.8 M in…

A: Concentration of Ca(OH)2 =0.45M Valume of KOH = 50ml Concentration of KOH =0.25M Concentration of…

Q: What is the pH of a 0.0550 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10.¹0)?

A: We have to find the pH of a 0.0550 M solution of hydrocyanic acid, HCN (Ka ).

Q: A scientist dilutes 50.0 mL of a pH 5.85 solution of HCl to 1.00 L. What is the pH of the diluted…

A: Given data,pH=5.85Volume of HCl=50mL=0.050LDilution=1.0LKw=1.0×10-14

Q: Hydrocyanic acid, HCN, is a weak acid (Ka = 4.02*10-10). If I dissolve 0.882 g of HCN in enough…

A: Given information is as follows: The amount of HCN = 0.882 g The volume of water = 600 mL The value…

Q: What is the pH of a 0.785 M solution of formic acid, HCHO2? The Ka of HCHO2 is 1.77 x 10-4.

A: In an aqueous solution of HCHO2, the dissociation of weak acid HCHO2 and autoionization of water…

Q: What is the pH of a system that is 0.40 M in NH3 and 0.80 M in NH4Cl? (Kb = 1.8 x10-5 )

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Q: Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11. What is the pH…

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Q: Given the weak acid, boric acid (H3BO3), calculate the pH and pOH of a 4M boric acid solution. Ka =…

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Q: For H2CO3, Ka1 = 4.3 x 10-7, K22 = 4.7 × 10-11 What is the pH of a 0.15 M solution of carbonic acid?

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Q: Calculate [H+] for a 3.00×10-4 M aqueous solution of cinnamic acid (HC9H7O2; Ka = 3.70×10-5)

A: The acid (say HA) dissociates in water to produce corresponding  ion and hydronium ions.          HA…

Q: What is the pH of a 0.10 M HSeO solution?  Ka = 1.3 × 10-4.

A: The dissociation reaction will be  HSeO ----> H+ + SeO-  Assuming y concentration of HSeO is…

Q: What is the pH of a 0.0490 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-1⁰)?

A: Concentration of HCN solution (c) = 0.0490 M Ka = 4.9×10-10 pH = ?

Q: . Calculate the pH of a 0.0368 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).

A: HNO2 is a weak acid and does not undergo complete dissociation in solution.

Q: What is the pH of an aqueous solution of 0.159 M sodium cyanide (NaCN)? (Kb of CN- = 2.5 x 10-5)

A: Given, The concentration of sodium cyanide (NaCN) = 0.159 M Kb for CN- = 2.5 x 10-5. pH is the…

Q: What is the pH of a 2.4 M solution of H2CO3? (Ka of H2CO3 = 4.3 x 10-7, Ka of HCO3- = 7x 10-11)

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Q: Calculate the pH of a 6.9 × 10¬³-M solution of H2SO4 ( -3

A: The pH is used to determine the acidity or alkalinity of a solution. Molarity of a solution is used…

Q: 4.0 g of baking soda (NaHCO3 , 84.02 g/mol) is fully dissolved in 100.0 mL water.  What is its pH?…

A: NaHCO3 is an amphiprotic species. That is, it can act as acid as well as a base.  The pH of such…

Q: What is the pH of a 0.01 M CH3COOH solution? (Ka= 1.74 x 10-5)

A: Given that  Ka of Ch3COOH is 1.74× 10^-5    Concentration of Ch3COOH is 0.01M

Q: What is the pH of a solution containing 100 mg/L acetic acid (CH3COOH)? (Ka=1.8x10-5)

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Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: What is the pH of a solution with [OH1-] = 1 x 10-8 ?

A: Since, pH represent the acidity of the solution. If pH less than 7 then solution is acidic. If pH =7…

Q: What is the pH of a 0.230 M solution of HF (Ka = 6.8 x 10-4)?

A: pH of a solution can be defined as the negative logarithm of [H3O+] ion concentration. HF is a weak…

Q: Given an aqueous solution of 0.05 M acetic acid (Ka = 1.8 x 10-5), the pH is approximately

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Q: What is the pH of an aqueous solution with .5 M NH3 & .45 M NH4Cl?  Kb=1.78 x 10-5

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Q: What is the pH of a 0.1088 M carbonic acid solution (Ka1 = 4.3 X 10-7)?

A: The concentration of the given carbonic acid solution = 0.1088 M Ka1 = 4.3 x 10-7

Q: What is the pH of a 0.173 M aqueous solution of sodium acetate, NaCH3COO? (Ka for CH3COOH =…

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Q: What the pH of a solution containing [H3O+] = 5.62 x 10-11 mol L-1 ?

A: Given that, for a solution [H3O+] = 5.62×10-11 mol/L. We have to calculate the pH of the solution.

Q: Determine the pH of a 2.79 M solution of acetic acid (CH3COOH, ka=1.8x10-5)

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Q: What is the pH of a 0.10 M solution of an acid that has a KA of 1.8 x 10–5?

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Q: What is the pH of 0.50 M aqueous ethylamine? (Ku of C₂H5NH₂ = 4.3 x 10-4)

A: The objective of this question is to calculate the pH of a 0.50 M aqueous solution of ethylamine…

Q: Lactic acid, HC3H5O3, is found in sour milk. What is the pH of 0.30 M lactic acid? This acid is a…

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Q: What is the pH of a 0.177 M diprotic acid solution (H2A)? Ka1 = 4.3 x 10-5 and Ka2 = 2.8 x 10-9.

A: The general equation for the dissociation of a diprotic acid (H2A) can be represented as follows:…

Q: What is the pH of an acetic acid, CH3COOH, solution that has an initial concentration of CH3COOH of…

A: Acetic acid is a weak monoprotic acid. In water it is dissociated as acetate ion and protons.

Q: If the K of a monoprotic weak acid is 1.4 x 10-6, what is the pH of a 0.14 M solution of this acid?…

A: Given : Ka of monoprotic acid (assuming HA) = 1.4 X 10-6  And Concentration of acid = 0.14 M Since…

Q: What is the pH of a 0.0580 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-1º)?

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Q: Süppose 10 mol HCIO4 (perchloric acid, a very strong acid) is dissolved in 1000 L of water. This…

A: We have to find pH of given solution

Q: Butyric acid  ( C3H7COOH) is a weak acid . What is the pH of a 0.0250 M solution of this acid. Ka =…

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Q: Consider a weak acid "HA". What is the pH of a 0.957 mol L-1 solution of HA? The KA of HA is 7.09 x…

A: The acid dissociation constant for the HA is = 7.09×10-7 The concentration of HCN solution is =…

Q: The pH of a 0.61 M aqueous solution of HNO2 (Ka = 4.6 × 10–4 at 298 K) is ____.

A: