A 0.100 M solution of the salt BHX has a pH of 8.00, where B is a weak base and X- is the anion of the weak acid HX. Calculate the Ka value for HX if the Kb value for B is 1*10-3

Q: 1. Calculate the pH of an acetate buffer prepared by dissolving sodium acetate (5.21 g) and acetic…

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Q: Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a…

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Q: What is the pH of a 0.20 M solution of a generic weak acid? The Kb value for this generic weak acid…

A: Given data  kb = 4.0 x 10-5 concentration, c= 0.20 M Formula used       OH- = kb×cpOH =…

Q: A 0.0560-g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution.…

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

Q: Caffeine (C8H10N4O2) is a neutral weak base and has a Kb= 4.1 x 10^-4. If you dissolve 85 mg in 5.00…

A: Given: Kb of Caffeine (Assuming B) is 4.1 × 10-4. Mass of B used = 85 mg = 0.085 g…

Q: Calculate the pH of a mixture that contains 0.26 M of HCOOH and 0.10 M of HC6H5O. The Ka of HCOOH is…

A: Answer :- Acid dissociation constant :-It is the equilibrium constant when dissociation of acid…

Q: A student was given a 0.15 M solution of an unknown diprotic acid H2A and asked to determine the Ka1…

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Q: A chemist titrates 250.0 mL of a 0.6025 M nitric acid (HNO3) solution with 0.4732 M NaOH solution at…

A: for the given titration, we have to calculate pH at equivalence point

Q: A chemist titrates 100.0 mL of a 0.3197 M potassium hydroxide (KOH) solution with 0.4567 M HBr…

A: KOH = strong base HBr = strong acid

Q: Given 0.10 M NaCn with a Ka value of HCN at 6.2 x 10-10 What is its pH?

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Q: What is the pH of a 80.0 mL solution which is 0.23 M in IO and 0.47 M in HIO? The Ka for HIO is 2.3…

A: When a weak acid(eg HIO) mixed with its conjugate base (ege IO-) they form a buffer solution. pH of…

Q: Calculate the pH of a buffer solution prepared by dissolving 0.6 mole of cyanic acid HCNO, and 0.5…

A: Answer :-  The pH of buffer solution prepared by dissolving 0.6 mol HCNO and 0.5 mol NaCNO in enough…

Q: An acid of the formula, HC6H5O, is a weak monoprotic acid. Its Ka is 1.1 x 10-10. A solution of this…

A: Given : Mass of HC6H5O = 14.5 g Volume of solution = 892 mL = 0.892 L…

Q: I mix 50.0 mL of 0.150 M CH3COOH with 10.0 mL of 0.100 M NaOH. Calculate the pH of the mixture.…

A: Henderson equation: pH = pKa + log[CH3COONa]/[CH3COOH] pKa = -logKa

Q: An acid HX is 25% dissociated in water. If the equilibrium concentration of HX is 0.30 M, calculate…

A: Given equilibrium concentration of HX is 0.30 HX is 25% dissociated in water

Q: In the laboratory, a general chemistry student measured the pH of a 0.474 M aqueous solution of…

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Q: |Ka for formic acid is 1.7 x 10-4 at 25°C. A buffer is made by mixing 425 mL of 0.428 M formic acid,…

A: Given: Ka of formic acid = 1.7×10-4 Concentration of formic acid (M1) = 0.428 M Concentration of…

Q: O. Calculate the Ka for a monoprotic acid, HX, if a 0.100000 M solution has a pH of 3.333. Write the…

A: The pH of a solution depends upon the concentration of H3O+ ions present in it. It is calculated by…

Q: The acid-dissociation constant (Ka) of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10. What is the…

A: NaCN    →     Na+   +    CN- CN-    +     H2O    ⇔     HCN   +     H3O+ The data given are- Ka of…

Q: C6H4NH2COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the…

A: Consider the given information is as follows; Concentration of C6H4NH2COOH = 8.0×10-2 MKa =…

Q: Calculate the pH of a 0.50 M HCOOH/ 0.60 M HCOOK buffer solution, and calculate the pH when 5.00 mL…

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Q: This curve represents titration of a. base with Kal < Ka2 b. base with Kbl < Kb2 C. acid with Kal <…

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Q: When 0.20 mol of NaOH is added to 0.50 mol of weak acid HX, in a total volume of 1.00 L, the pH of…

A: This acid - base reaction between NaOH and weak acid HX form a buffer solution. So we will use…

Q: A certain weak acid, HA, has a Ka value of 4.0x10-7. Calculate the percent ionization of HA in…

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Q: Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10,…

A: a) Given: Volume of HF=50 mL Concentration of HF= 0.2 M Concentration of NaH2BO3= 0.5 M Volume of…

Q: The value of Ka for acetic acid is 1.75 × 10—5. The pH of a 0.100 M solution of acetic acid is:

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Q: Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M…

A: Henderson – Hasselbalch equation is used to calculate the pH of a buffer solution. A buffer solution…

Q: 1. Acetic acid is a weak acid that when in an aqueous solution establishes the following…

A: Henderson - Hesselbatch equation PH = pKa + log SaltAcidKa = 1.8x10-5(Dissociation constant for…

Q: The weak acid HXO2 has a dissociation constant of Ka = 6.50 x 10-10. A lab worker prepares of 0.600…

A: We will calculate pH

Q: A 0.10 M solution of a weak acid HA has a pH of 2.80. What is the value of Ka for HA?

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Q: Ka

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Q: What will be the H+ concentration in a 0.25 M solution of a weak acid (HA), of Ka = 6.9x10-3 What…

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Q: What is the Ka or Kb expression for NH4Cl and Na2CO3? What is the value of Ka or Kb for both…

A: Salt hydrolysis: It is a reaction in which an acidic or basic solution is formed when one of the…

Q: Calculate the pH of a solution that contains 5.18 M of weak acid HA and 1.26 M NaA. The Ka of…

A: Given :  [HA] = 5.18 M  [NaA] = 1.26 M  Ka for Weak acid (HF) = 0.00063  To calculate :  pH of…

Q: A solution is made by mixing 150mL of 0.12 M HCN, 100 mL of 0.56 M NaOH and 75 mL of 0.78 M HCl.…

A: HCl dissociates into H+ and Cl-. Thus: [HCl] = [H+] Thus [H+] obtained from HCl =0.78 M Calculation…

Q: Calculate the pH of a solution that us 0.2 M NH3 (Kb=1.8 x 10^-5) and  M NH4NO3. Consider the…

A: pH is negative logarithm of concentration of H+

Q: An analytical chemist is titrating 71.3 ml of a 1.000M solution of formic acid (H,CO,) with a…

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Q: A 0.100 M solution of an acid, HA, has a pH = 1.52. What is the KA value for this acid?

A: Calculate the concentration of hydronium ion:

Q: Ka for hypochlorous acid, HCIO, is 3.0x10-8. Calculate the pH after 10.0, 20.0, 30.0, and 40.0 mL of…

A: Given: Concentration of NaOH= 0.100 M Concentration of HClO= 0.100 M Ka=3.0×10-8 To find: The pH of…

Q: after titrating

A: Mmol of Acid = 0.10 × 40    = 4.0 mmol Mmol of KOH = 20 ×0.20   = 4.0 mmol It forms Amphoteric salt,…

Q: A 0.0490 M  solution of an organic acid has an [H+] of 9.00×10-4 M . Using the values above,…

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Q: You have been observing an insect that defends itself from enemies by secreting a caustic liquid.…

A: The relation given by Henderson Hasselbalch for calculating the pH of the weak acid solution is…

Q: If a buffer solution is 0.240 M in a weak acid (Ka = 3.8 x 10-5) and 0.530 M in its conjugate base,…

A: Introduction Henderson - Hasselbalch equation gets used to calculate the pH for any buffer solution…

Q: The Ka of formic acid is 1.78x10-4. Compute the resulting pH of a 0.100 M solution of formic acid…

A: Since you have posted a question with multiple subparts, we will solve the first three subparts for…

Q: A 0.150 M solution of a weak acid has a pH of 2.75. What is the Ka value of this acid?

A: Given that, The concentration of a weak acid is C = 0.150 M. The pH of that 0.150 M solution of warm…

Q: In the laboratory, a general chemistry student measured the pH of a 0.522 M aqueous solution of…

A: Ka(experiment) = 5.9 × 10-5

Q: What is Ka for a weak monoprotic acid if a 0.020 M solution of the acid has a pH of 3.28 at 25°C?

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Q: Calculate the pH of a formic acid (Ka = 1.8 x 10-4) buffer solution that contains 0.35 mol HCOOH and…

A: Given:  Moles of HCOOH present = 0.35 mol Moles of HCOO- present = 0.28 mol Volume of the solution =…

Q: 100. mL of a 0. 10M solution of aqueous acetic acid is titrated using aqueous 0. 10M NaOH solution.…

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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.