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 5.11 O 4.95 7.15 6.23

Q: What is the pH of a solution when 4.9 g of ammonium bromide, NH,Br (M=98) , is used to make 200 mL…

A: Mass of NH4Br = 4.9 g Volume of solution = 200 mL K = 5.6E-10 pH =?

Q: What is the pH of the solution which results from mixing 25 mL of 0.30 M NH3 and 75 mL of 0.10 HCI?…

A: Given that : Volume of NH3 = 25 mL = 0.025 L Molarity of NH3 = 0.30 M Volume of HCl = 75 mL = 0.075…

Q: The % ionization of a 0.015 M aqueous solution of an acid is 0.14 at 25 °C. What is Ka of this acid…

A: Let the acid be HA. So it will disociate as H+ + A- . Let the concentration of acid be denoted as C…

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: 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: Calculate the percent ionization of nitrous acid in a solution that is 0.222 M (HNO 2) in nitrous…

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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: What is the pH of a solution that is 0.048 M in HA and also 0.0042 M in NaA? (Ka = 4.1 %3D x 10-6)

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Q: What is the pH of a 0.220 M solution of sodium cyanide (NaCN)? Ka for HCN is 4.9 x 10-9.

A: NaCN has one less hydrogen and corresponds to a conjugate base (a weak base). The credentials…

Q: Researchers have shown that hypochlorous acid (HCIO) generated by white blood cells kills bacteria.…

A: From Ka, α can easily be found. Then by multiplying the concentration with α, we can find the conc…

Q: Calculate the pH of a solution that is 0.410 M in HOCI and 0.050 M in NaOCI. [Ka(HOCI) = 3.2 x 10-8)…

A: Concentration of HOCl=0.410M Concentration of NaOCl=0.050M Ka(HOCl)=3.2 × 10^-8

Q: a) Calculate the pH of an aqueous solution of the salt NaA, which was made to a concentration of…

A: pH = 7 + (pKa + log C)/2 pOH = pKb + log [salt]/[base] pH + pOH = 14

Q: 4. What are the equilibrium concentrations of all species and the pH of a 0.20 M solution of HF…

A: The question is based on common ion effect.  Due to common ion effect of F- equilibrium of HF shift…

Q: QUESTIÓN 23 The Ka of HCIO is 3.00 x 10, What is the pH of a 0.0385 M aqueous solution of this acid?…

A: Given, the concentration of HClO =0.0385 MKa for the HClO =3.00×10-8we are asked to calculate the pH…

Q: 23 What is the pH of a solution composed of 0.20 M NH3 and 0.15 M NH.CI? (Kb NH3 = 1.8 x 10*)" (a)…

A: The pH and pOH of the solutions is the potential of H+ and OH- ions present in the solution. The…

Q: What is the pH of a 0.25M NaCH3COO solution? (the Ka value for acetic acid is 1.76 x 10^-5)

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

Q: What is the pH of a solution composed of 0.40M HOBr and 0.40M NaOBr. Ka of HOBr is 2.6x10-⁹ 9.12…

A: Given concentration of [HOBr] = 0.40M [NaOBr] = 0.40M Ka of HOBr = 2.6 * 10-9

Q: The pH value of 30 cm3 of a 0.2 M NaA solution is 9. What is the Ka of HA and the percent…

A: We have to calculate the Ka of HA and percentage ionization of HA.

Q: What is the pH of a 0.830 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The chemical equation may be written as: The given data is: Concentration of Ca(NO2)2 =0.830M Ka of…

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: What is the pH of a 0.375 L solution made with and 25.00 mL of 5.50 M HBRO (K, = 2.3 x 10 ) 2.775 g…

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Q: The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution.  (c)…

A: The reaction can be given as follows: HClO(aq)+NaOH(aq)→NaOCl(aq)+H2O(l) Molarity of HClO = 0.015 M…

Q: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively…

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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 the solution containing 0.1M sodium formate (NaHCOO) and 0.05M formic acid…

A: Required data to determine the pH of buffer solution using Henderson equation.

Q: What is the pH of the solution that is prepared when 121 g piperidinium chloride salt is dissolved…

A: Answer - The correct option is (d) 9.2 Solution -

Q: A solution is made with 3.825 g NH,CI, dissolved in enough water to make 625 mL of solution. If the…

A: First, we calculate the concentration of the solution. After that, we calculate the [OH-] with the…

Q: What will be the equilibrium tion of HA if the initial tion of monoprotic acid HA , (ka = 1 x 10^4)?…

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Q: Calculate the pH of a solution made by adding 0.11 g of solid NaOH to 275 mL of 0.250 M HNO2 (Ka =…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: What is the pH of 0.18 M sodium acetate solution? (Ka = 1, 8x10-5)

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Q: What is the pH of a 0.690 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: HNO2 ⇌ H+ + NO2- Ka = 4.5x10-4 = [H+][NO2-]/[HNO2] 4.5x10-4 = (x)(x)/0.690 - x  if we assume x is…

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 =…

A: Henderson-Hasselbalch equation explains the relationship between pH of solution and pKa of acid for…

Q: The pH of a 0.15 M solution of a weak monoprotic acid, HA, is 2.92. Calculate the Ka for this acid.…

A: Given data,Molarity of HA=0.15MpH=2.92

Q: The Ką of hypochlorous acid (HCIO) is 3 x 108. What is the pH at 25.0 °C of an aqueous solution that…

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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: What is the pH of 0.10 M NaF(aq). The Ka of HF is 6.8 x 10-4 2.08 14.92 8.08 5.92

A: The values are given as follows: A solution of NaF consists of F- and Na+ ions. Here, the F- is…

Q: Formic acid is in the venom of some ant species. What is the pH of a 0.35 M solution of formic acid…

A: Given: Concentration of formic acid HA = 0.35 M And Ka of HA = 1.78 × 10-4  The dissociation…

Q: Calculate the pH of a 0.100 M NaCH 3CO 2 solution. Ka for acetic acid, CH 3CO 2H, is 1.8 × 103.

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Q: Calculate the pH of a solution that is 0.50 in HF (Ka=7.2 x 10-4) and 0.95 in NaF.  a. 3.14 b.…

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Q: 7. Calculate the pH of a buffered solution that is prepared by dissolving 0.3 mol of NaHCO3 and 0.45…

A: The pH of an acidic buffer solution is given by the Henderson-Hasselbalch equation as…

Q: A weak acid (pka = 6.3) is dissolved in solution with a final pH = 5.7. At this pH, some of the acid…

A: Given the pKa of the weak acid(HA), pKa = 6.3  pH of the buffer solution, pH = 5.7

Q: Calculate the equilibrium molar concentration of a weak acid HA (154.5 g/mol) if 200 mg of that acid…

A: Weak acid - These are the acids that do not dissociate completely in water.  200mg of the weak acid…

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

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Q: 3) What is the pH of a 0.1OM solution of NaCN? The K, of HCN is 4.9 x 10-10. la. 2.85 b. 5.15 C.…

A: The salts that are formed from the strong acids and strong bases would not undergo hydrolysis. The…

Q: A 0.45 M aqueous solution of HBrO at 48°C is found to have a pH of 4.85 . What is the value of Ka…

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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: 3. A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to…

A: Buffer solutions The solution that resists any change in pH is known as buffer solution. pH of such…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.