What is the pH of a solution that is 0.32 M H(C6H5COO) and 0.12 M Na(C6H5COO)?   The Ka of H(C6H5COO) is 6.3 x 10-5

Q: Calculate the ph of 1.55 M CH3NH2. The Kb for CH3NH2= 4.4 x 10^-4

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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 of a 0.710 M solution of C5H5NHB (Kb of C5H5N is 1.7 x 10-9)?

A: pH is used to determine the concentration of hydronium ion.

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: Ka of HClO = 4.0 × 10-8 Concentration of the solution of NaClO = 0.089 M pH =?

Q: What is the pH of a solution of 0.300 M HNO, containing 0.180 M NANO,? (Ka of HNO2 is 4.5 x 10-4)

A: Given- Concentration of HNO2=0.300M Concentration of NaNO2=0.180M Ka of HNO2= 4.5×10-4

Q: Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4…

A: Given- Concentration of CH3NH2 = 0.35 M Kb = 4.4 × 10-4 To find - pH of solution Formula- pH = - log…

Q: What is the pH of 0.024M acetic acid solution at 25°C? (Ka=1.8×10^-5)

A: Given, [CH3COOH] = 0.024 M Ka = 1.8 × 10-5

Q: Calculate the pH of a 0.350 M solution of benzoic acid. Benzoic acid is a weak monoprotic acid with…

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Q: The hydronium ion concentration of an aqueous solution of 0.599 M formic acid, HCOOH (Ka =…

A: Given :  Concentration of HCOOH = 0.599 M  Ka = 1.8 x 10-4

Q: A 1.00 L solution contains propanoic acid (C3 H5 O2 H) with a concentration of 0.350 mol/L, and…

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Q: Determine the pH of a 0.22M NaF solution at 25 degrees Celsius. The Ka of HF is 3.5 x 10-5

A: We have to calculate the pH of 0.22 M NaF solution.

Q: Calculate pH for 0.0750 M C5H5NHCl (Ka=5.90 * 10^-6 for C5H5NH)

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Q: What is the pH of a 0.1250 M CH3NH3Br? Kb for CH3NH2 is 3.70e-4.

A: Given,  The pH of a 0.1250 M CH3NH3Br is : Kb for CH3NH2 is 3.70e-4.

Q: 6. Pyridine (P), a pesticide, is a weak base. Calculate the pH of a 0.0030 M solution of this base.…

A: In the given question we have to calculate the pH of Solution,  the Reaction of weak base,  C5H5N  +…

Q: The hydronium ion concentration of an aqueous solution of 0.591 M hypochlorous acid (K, = 3.50×10-8)…

A: [HClO] ( concentration of hypochlorous acid ) = 0.591 M  Acid equilibrium constant Ka = 3.50 * 10-8…

Q: Calculate the pH of 0.02354 M CH3 CO2 H and 0.1702 M NaCH3 C02. {Ka = 1.8 x10 °}

A: Given: [CH3CO2H]=0.02354 M [NaCH3CO2]=0.1702 M pH=? Ka=1.8 x 10-5

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 at 25 °C of water saturated with CO2 at apartial pressure of 1.10 atm? The Henry’s…

A: Concentration of CO2 can be calculated as follows: Where C is the concentration, KH  is the Henry’s…

Q: Which of the following is the pH of a solution with [H3O+] = 1.0 x 10-9? Select one: a. 1.00 b.…

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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: What is the pH of a 0.1966 M HCOOK? Ka for HCOOH is 1.74e-4.

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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 0.47 M weak base solution (Kb = 9.55 x10-5)?

A: Given information: concentration of weak base solution is 0.47 M Kb = 9.55 x10-5

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.10×10-3 M  solution…

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Q: What is the pH of a solution that has [H3O+] = 6×10^-12?

A: The pH of a solution is calculated as the negative logarithm of hydronium ion concentration and is…

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: -3 Calculate the pH of a 3.6 x 10-M solution of H2SO4 (Ka, = 1.2 x 10-2). pH =

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Q: Nitrous acid, HNO₂, has a Kₐ of 7.1X10⁻⁴. What are[H₃O⁺], [NO₂⁻], and [OH⁻] in 0.60 M HNO₂?

A: First of all we have to write the equation for nitrous acid.     HNO2+H2O⇔H3O++NO-2…

Q: What is the concentration of a solution of Ca1OH22 for which the pH is 11.68?

A: Ca ( OH)2 ------> Ca + 2 OH - pOH = 14 - 11.68 = 2.32 pOH = - log [ OH-] 2.32 = - log [OH-] [OH-]…

Q: What is the pH of a solution with H30+ =4.5 × 10^-5  M? 5.4 6.2 11.0 4.3

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Q: 5c. What is the pH of a solution which is 0.0400 M in potassium isocyanate (K* CNO") and 0.0300 M in…

A: Given, [K+CNO-] = 0.0400 M            [HOCN] = 0.0300 M As , K+CNO- is a salt it remains as…

Q: Determine the [H3O⁺] in a 0.265 M HClO solution. The Ka of HClO is 2.9 × 10-8.  Determine the pH of…

A: Given,Concentration of HClO = 0.265 MKa = 2.9 × 10-8The chemical reaction of dissociation of…

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

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Q: What is the concentration of hydroxide ion in a 0.76 M aqueous solution of hydroxylamine, NH2OH?…

A: Given data set: Molarity of NH2OH= 0.76 M Kw= 1*10-14 Kb = 1.1*10-8 we need to calculate the…

Q: What is the pH of 0.31 M diethylammonium chloride, (C2H5)2NH2Cl.  The Kb of diethylamine, (C2H5)2NH,…

A: The pH of the 0.31M diethylammonium chloride is given below

Q: The sodium salt of propanoic acid, NaCH3CH2CO2, is used as an antifungal agent by veterinarians.…

A: Given, Sodium sat\lt of propanoic acid NaCH3CH2CO2 Concentration Of propanoic acid = 0.72 M Kb of…

Q: (Q12) Hydrazoic acid (HN3) is a weak acid with a Ka of 2.5 x 10-5. What will be the equilibrium pH…

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Q: What is the pH of a solution that is 0.25 M CH3NH2 (methylamine) and 0.43 M CH3NH3Cl (methylammonium…

A: pH is the negative logarithm of hydronium ion. Henderson Hasselbalch equation for weak base: pKb…

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

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Q: what is the pH of an aqueous solution with [H3O+] = 2 x 10-14 mol L-1?

A: [H3O+] = 2 × 10-14 mol L-1  pH of the aqueous solution = ?

Q: Calculate the pH of 0.0985 M CH3COOH.  MM CH3COOH : 60.05 Ka = 1.8 x 10-5

A: Given data,Molarity of CH3COOH=0.0985MMolar mass of CH3COOH=60.05g/molKa=1.8×10-5

Q: The pH of a 1.50 M solution of anilinium chloride (C6H5NH3Cl) is _____.   Kb(C6H5NH2) = 4.3 × 10‒10…

A: Given,Kb(C6H5NH2) = 4.3 × 10‒10[C6H5NH3Cl] = 1.5 M

Q: Calculate the pH of 0.050 M aqueous solutions of the compounds below at 25 °C: a. NaOH b. CH3NH2…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: What is the pH of a 0.0680 M solution of hydrocyanic acid, HCN (Ка %3D 4.9 х 10-10)?

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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: Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5.

A: Given,Concentration = 0.461M.Ka = 6.5×10-5Then,

Q: The pH of a 0.20 M solution of a primary amine (RNH2) is 8.42.  What is the pKb of the amine?

A: RNH2 + H2O <---> RNH3+   +    OH-   Given datas ;  pH = 8.42 pOH = 14 - pH = 14 - 8.42 = 5.58…

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 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…