What is the k a of a monoprotic weak acid if a 0.728 M solution has a pH of 4.104?     1.17x108     6.21x10-9     7.88x10-5     8.52x10-9     1.17x10-9

Q: You use a pH meter to measure the pH of a solution that has a pH of 5.0. Determine the concentration…

A: The measure of the acidic and basic strength of any solution is given by its pH value. A strong acid…

Q: A 0.010 M solution of a weak acid, HA, has a pH of 3.10. What is the K, of the acid? 6.3 x 106 6.3…

A: pH is the negative logarithm of the hydronium ion concentration of a solution. Given:- pH = 3.10…

Q: KA

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Q: Which of the following is the weakest acid? OH A OH OMe B OH NO₂ C OH D OMe

A: The objective is to determine the weakest acoid.

Q: NH3 is a weak base (Kb = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: What is the pH of a solution that is 0.200 M ammonia (NH3) and 0.150 M ammonium chloride (NH4Cl)?…

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

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Q: For the diprotic weak acid H2A, Ka1 = 2.8 \times 10-6 and Ka 27.0 \times 10-9. What is the pH of a…

A: Please comment down for any doubt. I hope my answer helps you.

Q: Find the pH of a 2.0 M solution of H2SO4. Ka = 1.1 x 10^-2

A: Given :-  Concentration of H2SO4 solution = 2.0 M  Ka of H2SO4 = 1.1 × 10-2  To find :-  pH of…

Q: What is the acid-ionization constant, Ka, for this acid?

A: Given data contains, Concentration of HA is 0.200 M. pH is 2.210. The given chemical equation is,…

Q: A 2.0 M solution of a weak acid is found to have a pH of 5.5. What is the K₂ value of the weak acid?…

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Q: Calculate the [H+] in a 0.080 M solution of HCN, Ka = 6.2 × 10–10. 5.0 × 10-11 M 7.0 × 10-6 M 1.4 ×…

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Q: Which one of the following 1.0 M solutions would have the lowest pH?

A: D option is right. HF Ka provides a way to gauge the strength of an acid. Larger values signify…

Q: A 0.0720 M solution of a monoprotic acid is known to be 1.52% ionized. What is the pH of the…

A: Concentration of solution of monoprotic acid = 0.0720 M Percent ionization = 1.52%

Q: What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HCl and 30.0 mL solution…

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Q: The pH of a 0.0532 M solution of the weak acid HA is 3.24. What is K_{a} of this acid? O 6.3 * 10 ^…

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

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Q: What is the PH of a 0.13 solution of the salt NaX? Ka of HX= 1.5×10^-5

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Q: What is the k a of a monoprotic weak acid if a 0.533 M solution has a pH of 2.809? 4.50x10-6…

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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? O…

A: To find Ka value of a weak acid, first find out hydronium ion concentration and from that find out…

Q: What is the k a of a monoprotic weak acid if a 0.940 M solution has a pH of 3.607?     1.54x107…

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

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Q: Morphine, C 17H 19NO 3, is often used to control severe post-operative pain. What is the pH of the…

A: Which one of the following is correct answer

Q: Calculate the pH of the following aqueous solution:           0.40 M NH 4Cl (p K b for NH 3 = 4.74)

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Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: The pH of a 0.69M solution of alloxanic acid (HC4H₂N₂O) is measured to be 3.41. Calculate the acid…

A: pH = 3.41 Concentration  (c) = 0.69M Ka =?

Q: At 25 °C, how many dissociated OH ions are there in 1247 mL of an aqueous solution whose pH is 1.97?…

A: Given that At 25 °C, pH of the aqueous solution= 1.97 Volume of the solution= 1247 mL

Q: Calculate the K₂ for a monoprotic acid, HX, if a 0.100000 M solution has a pH of 3.333. The data is…

A: The given reaction is : HX     +     H2O      ⇔       X-     +     H3O+ The answer is as follows:

Q: sure your answer has the correct number of significant digits. Calculating the pH of a strong base…

A: Given :  Mass of Barium hydroxide = 216. mg  Volume of solution = 190. ml

Q: Consider the weak acid, HA, in water as shown in the reaction below. The [HA] initially is 0.3120 M…

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Q: -9 The acid dissociation constant K of hypobromous acid (HBrO) is 2.3 × 109. a Calculate the pH of a…

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Q: At 25 °C, how many dissociated H+ ions are there in 399 mL of an aqueous solution whose pH is 11.85?…

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Q: Which acid ionization constant would indicate the weakest acid? Group of answer choices 3.5 x 10–4…

A: In any aqueous solution, strong acids tend to get ionized in greater extent. Whereas weak acids get…

Q: find the ph of a .35 M aqueous acetic acid solution For CH3COOH Ka=1.8 x 10^-5 2.6 2.84 6.3 x 10^-6…

A: To predict: Need to find the pH of acetic acid.

Q: What is the pH of a 1.25 M solution of HClO? HClO (aq) + H2O (l) ⇌ H3O+ (aq) + ClO- (aq)…

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Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is…

A: Sodium acetate is a salt of weak acid (CH3COOH) and strong base(NaOH).CH3COONa →  CH3COO- +…

Q: A 0.600 M solution of NaX has a pH of 11.19. Which of the following could be NaX? Weak Acid Ka 4.9 x…

A: The objective of the question is to identify the correct compound NaX, given the pH of a 0.600 M…

Q: The Ka for lcarbonic acid is 1.8 × 10–5. Which of the following statements best describes the pH of…

A: The objective of this question is to determine the pH of a 0.0010 M solution of carbonic acid, given…

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.