A 0.25 M solution of a weak acid (HA) has a pH of 2.50. What is the Ka for this acid

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: How many moles of HA would need to be added to 481 mL of 0.816 M NaA to produce a solution with a pH…

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Q: An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium…

A: The equilibrium reaction given is, => HA --------> H+ + A-  Given : Initial concentration of…

Q: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: 8) A 0.185 M solution of a weak acid has a pH of 2.95. Calculate the acid ionization constant (Ka)…

A: A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant Ka…

Q: What is the ratio of concentrations of acetate ion and undissociated acetic acid in a solution that…

A: Ethanoic acid is a weak acid and the dissociation of acetic acid is given by: CH3COOH   ⇌  CH3COO-…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0176 M solution. The pH of the…

A: Given, Concentration of weak acid (C) = 0.0176 M pH of solution = 2.47 Dissociation constant (Ka) =…

Q: 69. A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calcu- late the acid ionization…

A: For weak acid : pH = 1/2pKa-1/2logC  Or, pKa = 2pH+logC ...(1)  Here, pH = 2.95 and C = 0.185 M…

Q: The pH of 0.259 M solution of an unknown acid is measured to be 2.353. What is the Ka of the acid?

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Q: Ka(experiment)

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Q: A solution of a weak acid has a concentration of 0.64 M and is found to have a pH of 3.77. What is…

A: The dissociation of a weak acid can be depicted as follows.           HA   +H2O ⇔    A-  +  H3O+I…

Q: The weak acid, H A, has a Ka value of 2.7E-5. Calculate the pH of the solution if the concentration…

A: Given: The concentration of weak acid HA =0.289 M Ka= 2.7 x 10-5 To Calculate: pH of the solution

Q: Calculate the Ka of weak acid.  The initial concentration of the weak acid is 4.93 x 10-4 M.  The…

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Q: 9) HB has a Ka of 5.2 x 10-5 and HC has a Ka of 4.6 x 10-4 . Which solution will have a lower pH,…

A: Given : Ka of HB = 5.2 X 10-5  Ka of HC = 4.6 X 10-4  And concentration of HB = concentration of HC…

Q: Acetic acid has a Kₐ of 1.8X10⁻⁵, and ammonia has a K(b) of 1.8X10⁻⁵. Find [H₃O⁺], [OH⁻], pH,…

A: (a) The acetic acid is a weak acid. The weak acid does not fully dissociate into its ions. We need…

Q: Calculate Ka for HA.

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Q: Solve the following problem, taking turns in your group to explain how to do the next step: What is…

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Q: 2) HF is as weak, monoptoric acid with a Ka value of 6.6x104. Calculate the pH of a 0.25 M solution…

A: Weak acid and its salt will form buffer solution.  Note: As per our company guideline we can answer…

Q: A 0.215 M solution of an unknown monoprotic acid has a pH of 4.87. What is the Ka for this acid

A: Given: Initial concentration of monoprotic acid solution = 0.215 M pH of solution = 4.87

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0111 M solution. The pH of the…

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Q: The weak acid HA is determined to be 8.32% dissociated when the initial concentration of HA is…

A: Initial concentration of HA = 0.0300 M Degree of dissociation = α = 8.32 % = 0.0832

Q: An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium…

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Q: calculate Ka and the percent ionization of an acid HA given that 0.70 M of HA has a pH of 4.00

A: Weak acid are those acid which does not dissociate completely in aqueous solution.

Q: A 0.60 M solution of a weak acid, HA, has a pH of 3.41. What is the percentage ionization of the…

A: ★ Answer : percentage of ionization of the acid is 0.064%

Q: 8.0 x 10-10

A: Using pH formula for weak acid, pH = 1/2(pKa - logC) 4.70 = 1/2(pKa - log(0.50)) pKa = 9.10

Q: If the pH of a 0.800 M solution of the acid HA is 3.45, calculate 1) the % ionization of this acid…

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Q: 10. The pH of 0.25 M aqueous solution of a weak acid HA is observed to be 4.15. Determine the acid…

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Q: Given that the Ka of a monoprotic acid HA is 3.20 x 10-7 , and the acid HA concentration is 0.751 M,…

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Q: If a 0.8M solution of weak acid, HA, has a pH = 2.8, calculate the Ka of the acid.

A: The pH of a solution denotes the -ve logarithm of hydronium ion concentration in moles per liter.…

Q: Calculate the pH value of 0.00 * ? acid at 25 C if Ka=0.0O00018 3.1

A: Given:  0.001M acetic acid at 25C if Ka = 0.000018   To find: pH value of 0.001M acetic acid at 25C…

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: An acid (HA) dissociates as follows: HA → H* + A minus Arrow should be interpreted as an equilibrium…

A: Acid dissociation constant is commonly known as Ka , it measures the strength of acid in solution.

Q: An acid HA has a Ka of 1.00 x 10-7. Calculate the pH of a 0.100 M solution of its conjugate base.…

A: Given: Concentration of conjugate base of weak acid HA i.e. A- = 0.100 M And Ka of HA = 1.00 × 10-7…

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 Ka of an acid, HX, whose ionization is 31% when CHX= 0.60 M (Note that the %…

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Q: A 0.037 M solution of a weak acid (HA) has a pH of 4.59. What is the Ka of the acid?

A: Given :-  Concentration of weak acid = 0.037 M  pH of solution = 4.59  To calculate :-  Value of Ka

Q: The pH of 0.250 M hydrofluoric acid is 2.036. Calculate the value of Ka for hydrofluoric acid.

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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: If a 0.59 M solution of a monoprotic acid HA has a pH of 4.57, what is the Ka value of the acid HA?

A: Concentration of Acid HA = 0.59 M pH = 4.57     ICE Table:…

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: An acid (HA) dissociates as follows: HA – H* +A minus Arrow should be interpreted as an equilibrium…

A: pH is defined as the negative logarithm of concentration of H+ ion.

Q: A given acid whose concentration is 0.492 molar has a pH of 3.38. What is the KA for this acid? 3.5…

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Q: Consider 1M solutions of each of the following acids (with their Ka values). Which solution would…

A: The question is based on the concept of acidity. we have to identify which of the given acid has…

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: A 0.10 M solution of a weak acid HA has a pH of 4.00. What is the value of Ka for HA? Hint: set up…

A: Given concentration of a weak acid is---- 0.10M pH of the weak acid HA is---- 4.00 What is the value…

Q: what is the ph of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? (Ka for…

A: Given : concentration of acetic acid = 0.50 M concentration of sodium acetate = 0.75 M and Ka of…

Q: An acid (HA) dissociates as follows: НА - H* + A minus Arrow should be interpreted as an equilibrium…

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Q: The weak acid, HA, has a Ka value of 2.6E-5. Calculate the pH of the solution if the concentration…

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.