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

Q: What is the pH of a 5.0×10-2 M solution of KOH at 25 °C?

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Q: Consider a weak acid "HA". What is the pH of a 0.626 mol L¯' solution of HA? The KA of HA is 6.5 x…

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Q: What is the pH of a solution that contains 0.10 M HCl and 0.10 M acetic acid (HC2H3O2)? Ka for…

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Q: What is the pH when the [OH-] = 4.26 x 10-2 M at 25 oC?

A: 1- First we need to calculate the pOH of the solution :  We know that,  pOH = -log[OH-]  pOH = -log(…

Q: What is the pH of 1.65e-3 M Ba(OH)2?

A: pH = 11.52  SOLUTION :-  14 = pH + pOH  pOH = - log [OH-]   1.65e-3 M Ba(OH)2  1 mol of Ba(OH)2…

Q: If the Ka of a monoprotic weak acid is 5.8 × 10-6, what is the pH of a 0.47 M solution of this acid?

A: Given: Ka=5.8×10-6 Molarity of acid = 0.47 M

Q: What is the pH of 0.75 M HC2H302 solution? K.= 1.8 x 105 and Kn=1.00 x 10-14 HC2H3O2 + H2O H3O* +…

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Q: What is the pH of a 3.76.10-8 mol.L-1 NaOH solution?

A: From the sodium hydroxide concentration, hydroxide concentration can be calculated.…

Q: determine the pH of 0.251M acid HA solution. The Ka of the HA is 3.77x10^-7

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Q: What is the pH of 3.78 *10^-2 M nitric acid in aqueous solution ?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

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: Calculate the pH of a 3.12×10-3 M  solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

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

A: Given concentration of CH3COOH = 1.75 × 10-5

Q: what is the pH of 0.12795M CH3COOH solution? Ka=1.8x10^-5

A: We have to calculate the pH.

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.450 M  solution of methylamine?

A: Methylamine, CH3NH2 is a weak base which undergoes partial dissociation in aqueous medium. Let the…

Q: What is the pH of a 0.17 M weak acid solution? The KA of the weak acid is 2.1 x 10-5.

A: Given :-  Initial concentration of weak acid = 0.17 M  Ka for acid = 2.1 × 10-5  To be calculated :-…

Q: What is the pH of a 3.6×10-2 M solution of KOH at 25 °C?

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Q: What is the pH of a 0.36 M Sodium acetate solution (CH3COONa)…

A: Sodium acetate is a salt of a weak acid (CH3COOH) and a strong base (NaOH). Therefore, the pH…

Q: What is the pH value of 1x10-3 M CH3COOH solution? (Ka: 1.75x10-5)

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Q: Determine the pH

A: The scale which is used to analyze the acidity and basicity of an aqueous solution is called as pH…

Q: What is the pH of a solution of 0.85M HC2H3O2 and 0. 65M NaC2H3O2? The Ka for HC2H3O2 is 1.8 x 10^-5

A: Buffer Solution :- Buffer solution is prepared using weak acid and it's conjugate base of the weak…

Q: If the Ka of a monoprotic weak acid is 3.4 × 10-6, what is the pH of a 0.30 M solution of this acid?

A: The dissociation of a weak acid is written as:

Q: What is the pH of a solution containing 4.5 x 10-5 M HCl?

A: Given : Concentration of HCl = 4.5 X 10-5 M

Q: What is the pH of a 3.9×10-2 M solution of KOH at 25 °C?

A: KOH ionizes in aqueous solution as,                          KOH (aq)       -----> K+ (aq)   +…

Q: What is the pH of a 0.0620 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10¬1º)? %3D

A: Given data,Molarity of HCN=0.0620MKa=4.9×10-10

Q: What is the pH of (3.21x10^-1) M C5H5NHBr?

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

Q: The Ka for hydrofluoric acid is 7.1 × 10−4. Calculate the pH of a 0.15-M aqueous solution of…

A: pH: It is defined by saying that power of hydrogen present in any solution. It can be calculated…

Q: The Ka for formic acid (HCO2H) is 1.8x10-4, What is the pH of a 0.20M aqueous solution of sodium…

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Q: a) What is the pH and pOH of 0.001 M NaOH solution, which is the strong base? b) The Ka value of…

A: pH + pOH = 14 pOH = -log [OH-] For a weak acid: [H+] = (Ka x C)1/2 Where, C = molar concentration

Q: The pH of 1.0 x 10 -11 M of NaOH is اخترأحد الخيارات а. 10 O b. 4.0 O C. 7.0 O d. 6.0 O e. 11.0 O

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Q: What is the pH of 0.80 M methylamine (CH3NH2). Kb = 4.4x10-4.

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Q: What is the pH of a 7.8×10-5 M Ca(OH)2 solution?

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Q: The organic acid RCOOH has a Ka = 4.1e-5. What is the pH of a 0.50M aqueous solution of this acid?

A: given, Ka = 4.1e-5 [RCOOH]= 0.50M

Q: What is the theoretical pH of a 0.10 M NH4Cl solution when the Kb for NH3 is 1.8 x 10^-5?

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Q: What is the pH of a 1.00 x 10-9 M solution of NaOH at 25 oC?

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Q: For H2CO3, Ka1= 4.3 x 10^-7, Ka2= 4.7 x 10^-11. What is the pH of a 0.28 M solution of carbonic…

A: H2CO3 is a weak acid.  pH = 0.5pKa - 0.5logC ....(1) Here, pKa1 = -logKa1 = -log(4.3*10^-7) = 6.37…

Q: What is the pH of a 0.862 M NH3 solution that has a Kb = 1.8 x 10-5?

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Q: what is the pH of a 7.1 x 10^-3 M solution of H^+?

A: Given : [H+ ]  = 7.1  x 10-3 M

Q: What is the Ka of hydrazoic acid if a 0.020 M hydrazoic acid aqueous solution has a pH of 3.22?

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Q: Calculate the pH of the following aqueous solutions at 25°C: (a) 9.5 × 10-8 M NaOH, (b) 6.1 × 10-2 M…

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Q: What is the pH for a solution at 25 °C that has a OH" concentration of 3.08 ×10-4 M?

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Q: A 1.00 L solution contains propanoic acid (C3 Hs O2 H) with a concentration of 0.210 mol/L, and…

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Q: How many milligrams of CH3COOH (fw 60) should be added to 250 mL of water to get pH 3. K. = 1 x 10-5

A: CH3COOH is weak acid in aqueous solution. It will dissociate in solution as below-

Q: . What is the pH of a solution consisting of 0.85M HC2H3O2 and 0.60M NaC2H3O2? Ka of HC2H3O2 = 1.8 x…

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Q: Calcualtw the pH of a 0.217 M HC7H5O2 aqueous solution. Ka for HC7H5O2 is 6.5 x 10^-5.

A: pH of an acid is equal to negative logarithm of concentration of H+ ions.

Q: What is the hydronium ion concentration [H3O+] of a 0.010 M acetic acid solution in water? (Ka for…

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Q: What is the pH of a solution with [OH-] = 5.54 x 10^-5

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Q: What is the pH of a solution that is 0.11 M CH3NH2 (methylamine) and 0.15 M CH3NH3Cl (methylammonium…

A: Since the solution is having weak base CH3NH2 and its conjugate acid salt CH3NH3Cl  Hence the…