What will be the pH of a solution containing 0.200 M NaH2PO4 and 0.200 M Na2HPO4? Ka(NaH2PO4) = 6.2 x 10^8

Q: What is the pH of a 0.265 M  solution of H2SO4? Ka2 = 1.20×10–2

A: Given the molarity of   H2SO4 = 0.265 M   H2SO4 is a strong diprotic acid with high Ka1 value and…

Q: What is the pH of a 7.041 x 10^-6 M HCIO4 solution?

A: Given , concentration of acid solution = 7.041 x 10^-6 M   That means,  [H+] = 7.041 x 10^-6 M

Q: Calculate the formate ion concentration and pH of a solution that is 0.050 M in formic acid (HCOOH,…

A: Since HCOOH is a weak acid and HNO3 is a strong acid Hence HNO3 will dissociate completely into ions…

Q: Calculate the pKa of hypochlorous acid. The pH of a 0.015 M  solution of hypochlorous acid has a pH…

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Q: Calculate the pH of a 0.053 M NaF solution. (Ka for HF = 7.1 x 10−4.)

A: NaF is a salt of strong base (NaOH) and weak acid (HF)

Q: What is the hydronium ion concentration in an aqueous nitric acid solution with a pH of 3.570?

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Q: Calculate the pKa of the weak acid HA, given that a solution of 0.65 M HA and 0.85 M NaA has a pH of…

A: The formula for calculating pKa of an acid with the given values of pH and concentrations of HA and…

Q: What is the pH of a 0.050M solution of (CH3)3NHC1?

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Q: What is the pH of a solution containing both 0.10 M CH₃COOH and 0.20 M CH₃COONa? The Ka of CH₃COOH…

A: We have to predict the pH of the given solution.

Q: Calculate the pH of a .10 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4.

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Q: What is the hydronium-ion concentration of a 2.13 ✕ 10−4 M solution of p-bromobenzoic acid,…

A: Interpretation: The hydronium-ion concentration of a 2.13 ✕ 10−4 M solution of p-bromobenzoic acid,…

Q: Calculate the pH of a solution containing 0.3 M HCOOH and 0.1 M HCOO (pKa of HCOOH = 3.76)

A: Concentration of HCOOH (Acid) = 0.3 M  Concentration of HCOO- (conjugate base of acid) =  0.1 M  pKa…

Q: What is the pH of a 0.22M NaH2PO4 solution?

A: NaH2PO4 is a weak.Ka for NaH2PO4 is 6.23×10-8.Calculate concentration of H3O+:

Q: The equilibrium constant for the following reaction: NH3(aq) + H20(e) Z NH4*(aq) + OH (aq) is: Keq =…

A: Equilibrium constant is the ratio of concentration or pressure of products to that of reactants.

Q: Calculate the pH of a 0.20 M solution of NaC2H302. HC2H302 has a Ka=1.8 x 10. O a. 7.00 O b. 4.98 O…

A: i would go for option b- 4.98 as acid concentration is missing so i am unable to give you a solution…

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 0.193 M w. acid HA solution? Ka = 6.61 x 10−6?

A: The acid is weak so it weakly dissociates in the solution. That is it gives an H+ ions slowly in to…

Q: What is the pH in a 0.0320 M aqueous solution of formic acid (HCOOH)? (For HCOOH, Ka=1.8 x 10–4)

A: HCOOH is a weak organic acid. It dissociates into formate ions and hydrogen ions. The ICE table for…

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

A: pH of a 0.48 M solution of carbonic acid = 3.35

Q: The pH of a 0.10 M solution of Ni(NO3)2 is 5.0. Calculate the acid ionization constant of Ni(H 2O)…

A: [Ni(H2O)6]2+ is a Bronsted- Lowry acid. It releases H3O+ in solution.The acid ionization reaction is…

Q: Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed…

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Q: Calculate the pH of a 0.010-M solution of iodic acid (HIO3, Ka = 0.17).

A: Molarity of Solution = 0.010M Ka of Acid = 0.17 We have to find the pH of the solution of iodic…

Q: Calculate the pH of a 0.20 M solution of sodium acetate (NaCH3COO) given that the Ka of acetic acid…

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Q: 3. Calculate the pH of a solution containing 0.10 M H3BO3 and 0.18 M NaH2BO3 Ka = 5.81 X 10 10

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Q: Calculate the pH of a 0.100 M NaHCO3 solution.

A: The pH of a given solution can be defined as the measure of its basicity or acidity. More the pH…

Q: Calculate the pH of a solution that is 0.0400 M in  a. NaH2PO4 b. NaH2PO3 c. NaHS

A: pH is equal to the negative logarithm of hydronium ion. Given data: Concentration of all given…

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: Calculate the pH of a 0.0101 M aqueous solution of formic acid (HCOOH, Ka = 1.8E-4). pH =

A: For weak monoprotic acid ( HCOOH) : pH = 0.5 x (- log Ka - log C ) pH = 0.5 x ( - log 1.8 x 10-4 -…

Q: What is the pH of a 0.190 M  solution of sulfurous acid? Given: Ka1 = 1.70×10–2, Ka2 = 6.20×10–8

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Q: What is the hydronium ion concentration in an aqueous hydroiodic acid solution with a pH of 3.970?…

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Q: What is the pH of a 0.35 M solution of hydrofluoric acid with a K, of 6.6 x 104? 3.23 O 1.82 O 5.47…

A: Given: Concentration of HF acid = 0.35 M Ka of HF = 6.6×10-4

Q: Calculate the pH of a 0.20 M solution of NH4NO3. (Kb(NH3) = 1.8 x 10)

A: Salt of Weak base and Strong acid  pH = 7 - 1/2 ( pKb  - logC )

Q: Determine the hydroxide ion concentration and pH of 0.0942 M hypochlorous acid solution. Ka = 2.85 x…

A: Concentration of hypochlorous acid (HOCl) solution = 0.0942 M Ka of HOCl = 2.85 * 10-8

Q: Calculate the pH and percent ionization of 0.05 M acetic acid Ka = 1.8 x 10 -5. %3D

A: Given, Concentration of acetic Acid (C) = 0.05 M Ka for acetic acid = 1.8 × 10-5  pH = ? Percent…

Q: Calculate the pH of a solution resulting from the addition of 50.0 mL of 0.30M HNO3 to 50.0 mL of…

A: Nitric acid which is a strong acid on undergoing a reaction with ammonia will form a salt of…

Q: Barbituric acid, HC4H3N2O3, is used to prepare various barbiturate drugs (used as sedatives).…

A: Given data: The concentration of Barbituric acid solution [HC4H3N2O3]=0.10 M. The acid dissociation…

Q: What is the pH of a 0.270 M  solution of H2SO4? Ka2 = 1.20×10–2

A: Here given, Ka2 = 1.20 × 10-2 Concentration of  H2SO4 = 0.270 M

Q: Arrange the following in order of INCREASING acidity. I. II. II. IV. ... CI CI OH OH CI CI

A: Correct option is • B    I < III < Iv < II Acidiity depends on the conjugate base…

Q: Is Mg(OH)2 a acid, base, or neither?

A: According to the Arrhenius concept of acids and bases :-  Acids donate H+ ions in water and bases…

Q: f) Calculate the pH of the following solutions: (i) A 0.045 M solution of sulphuric acid. (ii) A…

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Q: What is the pH of a solution of 0.0745 M NACH3O2 ? Ka = 1.8 x 10

A: Given: Concentration of NaC2H3O2, [NaC2H3O2]= 0.0745M Ka = 1.8 x 10-5

Q: 3. Write a net ionic equation for the equilibrium that causes the solution of KHTar in water to be…

A: The potassium acid tartrate, KHTar salt is obtained from neutralization reaction of tartaric acid by…

Q: Calculate the pH of a solution that is 0.250 M in HClO4 and 0.125 M in CH3COOH (Ka = 1.8 x 10-5)

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Q: Determine the Ph of a 0.020 M solution of oxalic acid, H2C2O4. What is the concentration of C2O4 ion…

A: Oxalic acid is diprotic acid and Ka1 = 6.5 * 10-2 and Ka2 = 6.1 * 10-5 [Oxalic acid] = 0.020 M…

Q: Calculate the pH of 0.0154 M NaN3. (Ka of HN3 = 1.9 x 10-5)

A: NaN3 is a salt of weak acid (HN3) and strong base (NaOH). We know, the pH of salt, which is formed…

Q: Calculate the pH of a 4.23×10-2 M solution of hypochlorous acid at 25°C. Ka for hypochlorous acid is…

A: We have to calculate the pH of a 4.23×10-2 M solution of hypochlorous acid ( HOCl) at 25°C. Ka for…

Q: Calculate the concentration of an aqueous solution of Ca1OH22 that has a pH of 10.05.

A: Since Ca(OH)2 is insoluble salt  Hence molar solubility of Ca(OH)2 = concentration of Ca(OH)2 in…

Q: When preparing 0.075 M KCN solution, the equilibrium constant (Ka) was found to be equal to 49 x…

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Q: What is the hydronium-ion concentration of a 2.63 ✕ 10−4 M solution of p-bromobenzoic acid,…

A: Given, initial concentration of BrC6H4COOH = 2.63 ✕ 10−4 M The ionization of BrC6H4COOH takes place…