Explain what happens to the concentration of hydrogen ions in anaqueous solution when you add a base and cause the concentrationof OH-to rise to 10-3. What is the pH of this solution?

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 a solution which is 0.021 M in weak base and 0.039 M in the conjugate weak acid…

A: We have a buffer system of weak base (0.021M) and conjugate weak acid (0 .039M) . We also have the…

Q: 1. Calculate the pH of each of the following solutions of a strong acid in water. a. 0.10 М НСІ b.…

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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: 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: 3. 0.9206 grams of acetic acid is dissolved in enough water to make 60.0 mL of solution. Solve for…

A: Molarity :-  The number of moles of solute dissolved in 1 litre of solution is defined as molarity…

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: What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,l? (Kb of CH;NH, is 4.4 x…

A: This is a basic buffer solution. A buffer resist the change in PH of the solution.

Q: What is the pH of a 0.350 M triethylamine, (C2H5)3N, solution?             Kb for triethylamine is…

A: Given, 0.350 M triethylamine  Kb for triethylamine is 5.3 *10-4

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: Calculate the pH and the pOH of these solutions:   (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH =   pOH…

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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: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: What is the pH of a solution with [OH1-] = 1 x 10-8 ?

A: Since, pH represent the acidity of the solution. If pH less than 7 then solution is acidic. If pH =7…

Q: What is the pH of 0.030 M aqueous formic acid (Ka of HCO2H = 1.8× 10^-6)

A: Formic acid dissociates as follows:                               HCOOH (aq) ⇌ HCOO- (aq) + H+ (aq)…

Q: What is the PH for a solution with [OH^-]=1.0X10^-6??

A: The relationship between the pH and pOH is as follows:                   pH+pOH =14 The formula for…

Q: Calculate the pH of a solution that is 0.155 M in NH3 acid and 0.255 M in NH4Cl. The Kb of ammonia…

A: Weak acid and its conjugate base forms a buffer solution similar to a weak base and its conjugate…

Q: 5. Calculate the pH of a solution containing 0.1 M of acetic acid (CH;COOH). The pKa of acetic acid…

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Q: Calculate the ph of a solution that is made by dissolving 6.45g of NH4Cl(53.49g/mol) in enough water…

A: First calculate molarity by mole/volume. Then use weak base concept to get pH

Q: Calculate the pH of a 0.15M solution of sodium acetate (CH3COONa). What is the percent hydrolysis?…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: 5. Write equations to illustrate the amphoteric nature of H2PO (aq) and label the conjugate acid-…

A: Write equations to illustrate the amphoteric nature of H2PO- (aq) and label the conjugate acid-base…

Q: What is the PH of a 0.01 M solution of salt NaA, where A- is the anion of an acid whose ionization…

A: Given that,  Concentration of salt NaA, = 0.01 M Ionisation constant Ka   = 10-6 pH of the given…

Q: When red wine is fermented with bacteria, the result is red wine vinegar! Fermentation converts the…

A: pH is equal to the negative logarithm of hydronium ion. pH=-log(H3O+) Henderson Hasselbalch…

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: The Ka of acetic acid is 1.80 x 10-5.  A. What is the pH of a 0.0010 M solution of acetic acid? B.…

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Q: Which of the following is the example(s) of acid-base reaction? H H `H H -Br II IV OH H-CI OH

A: Acid- The species which is able to donate H+ ion.   Base-  The special which is able to accept H+…

Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…

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Q: (Q25) A buffer solution is prepared by adding 0.797 moles of formic acid and 0.866 moles of sodium…

A: ★ Answer : pH of the solution will be 4.027  ★ Solution :

Q: The Ka of propanoic acid (C,H,COOH) is 1.34 x 10-5. Calculate the pH of the solution and the…

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Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

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Q: Calculate the pH of a 0.021 M NaCN solution at 25 degrees Celsius. Ka (HCN) = 4.9 x 10^(-10). You…

A: Given, Concentration of NaCN solution = 0.021M. Ka(HCN) = 4.9*10-10. The hydrolysis reaction of NaCN…

Q: What is the pH of a 0.010M solution of acetic acid? Ka for acetic acid is 1.8 x 10-5

A: Given :-  [CH3COOH] = 0.010 M  Ka = 1.8 × 10-5  To calculate :-  pH of solution     Ka is the ratio…

Q: The Ka of a weak acid is 5.42 x 10-5. What is the pKb of its conjugate base?

A: Ka = 5.42 × 10-5 (given )  pKa = - log [Ka]  pKa = - log ( 5.42 × 10-5 )  pKa = 4.266

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: NH3 is a weak base (K, = 1.8 x 10-5) and so the salt NH¼C1 acts as a weak acid. What is the pH of a…

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Q: What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5

A: Given, Molar concentration of NH4Cl = [NH4Cl] = 0.1 M Base dissociation constant of NH3 = Kb = 1.8…

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 0.20 M solution of sodium acetate? The Ka for acetic acid is 1.8x10-5 ?

A: Given, Concentration of sodium acetate = 0.20 M Ka of acetic acid = 1.8 x 10-5 Formula used, [OH-] =…

Q: What is the pH for 2.4 M ammonium chloride aqueous solution (ammonium hydroxide, Kb=1.8×10-5)?

A: Ammonium chloride,  NH4Cl  dissolves in solution to form ammonium ions  NH4+  which act as a weak…

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: Determine the pH of a solution by adding 0.23 mole formic acid and 0.17 mole of sodium formate in…

A: Here formic acid is a weak acid and sodium formate is an salt of weak acid so they both combine to…

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: For acetic acid, Ka=1.8 times 10^-5. Calculate the pH, [OH]-, and [HC2H3O2] in a 0.534 M solution of…

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Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

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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 l.6M Soluten of Ascorble Acid, th C HG OG Kaz -5 = 8.0 x10, Ke=1.6A 10-12)

A: Given: Concentration of H2C6H6O6 = 1.6 M Ka1 of H2C6H6O6 = 8.0 × 10-5 And Ka2 of H2C6H6O6 = 1.6 ×…

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

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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.