The value of Ka for acetic acid , CH3COOH , is 1.80×105. Write the equation for the reaction that goes with this equilibrium constant. (Use H3O* instead of H*.) + ? +

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

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

Q: Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid…

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Q: KA

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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: All of the following are weak bases except:  A. Al(OH)3 B. Mg(OH)2 C. NH3 D. B(OH)3

A: The compound that is weak base has to be identified.

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: Using Brønsted-Lowry definitions, designate each of the following as a strong base (SB), a weak base…

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Q: What is the % ionization of a solution of 0.20 M benzoic acid, C,H,COOH (K¸ = 6.6 x 10 ')? Would a…

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Q: A weak acid has Ka of 4.82 x 10-5.  What is pKa for this weak acid? Enter a numerical value in the…

A: Given: Ka = 4.82 × 10-5

Q: Propanoic acid HC3H5O2, has a Ka of 1.3 x 10-5. What is the [H3O+] in a (1.51 x 10-1) M solution of…

A: The ionization of Propanoic acid HC3H5O2 takes place as,                             HC3H5O2 (aq)  +…

Q: The Ka for benzoic acid is 6.5 × 10¯. Calculate the pH of a 0.10 M benzoic acid solution.

A: Benzoic acid is monoprotic and a weak acid. It partially ionize in solution to produce C6H5COO- and…

Q: a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; +…

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Q: Calculate the Ka for an unknown monoprotic acid HX, given that a solution of 0.10M LiX has a pH of…

A: In this question we have to calculate the Ka of monoprotic acid from the following data given.…

Q: A tablet containing 500 mg of aspirin was dissolved in enough water to make 100 mL of solution.…

A: Given, Mass of aspirin, C9H8O4 = 500 mg = 0.500 g     (1 mg = 0.001 g) Volume of solution = 100 mL =…

Q: For a given acid, Ka is 7.2  x 10−4. This means that it is: a strong acid B a weak base C a weak…

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Q: A 0.55 M aqueous solution of HBRO is 4.48. What is the value of Ka for this acid? O 1.1 x 10-9 2.0 x…

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Q: Calculate the pOH of a 1. 0-M solution of methylamine (Kb = 4.38x10-4) methylamine (CH3NH2) is a…

A: Weak base does not dissociate 100%              CH3NH2    +   H2O     →    CH3NH3+     +     OH-…

Q: In the laboratory a student measures the percent ionization of a 0.429 M solution of formic acid ,…

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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: A 0.15 M solution of an acid found in milk has a pH of 2.80. What is the percentage ionization of…

A: HA → H+ + A- The formula to calculate the pH is, pH= -log[H+] Therefore rearranging the formula let…

Q: arbonic acid is an example of weak acid. Calculate the Ka of the carbonic acid (H2CO3) based on the…

A: Acid dissociation constant can be determined by dividing the equilibrium concentration with initial…

Q: In an analysis carried out with water (H2O) at 90 °C, a chemist found an amount of hydroniums (H3O+)…

A: Given :-  Concentration of hydronium ion at 90°C = 5×10-7 mol/L  Concentration of hydroxide ion at…

Q: You have 70 ml of 0.1 M HA, after adding 30.0 ml of 0.1 M NAOH, the pH is 5.0 what is the Ka of HA?…

A: We are given an Acid HA and a base NaOH. We have to find the ka of the acid. We are also given the…

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: Write the chemical equation and the Ka expression for the ionization of each of the following acids…

A: Given: Two compounds, (a) HBrO2 (b) C2H5COOH

Q: Identify Ca(OH)2(aq)Ca(OH)2(aq) as an acid or a base. Write a chemical equation showing how this is…

A: According to Arrehenius theory , base is a substances that contain OH group and produce OH- ions in…

Q: 7. The ka for acetic acid is 1.0 x 10.5. Is acetic acid a weak or a strong acid?

A: Strong acids completely dissociate in aqueous solution (Ka > 1, pKa < 1).

Q: A 0.50 M solution of an acid HA has pH = 2.24. What is the value of Ka for the acid?

A: Given, molarity(M)=0.50M. The pH of the acid =2.24 To  calculate, Ka(dissociation constant of the…

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: 14.What is the k a of a monoprotic weak acid if a 0.213 M solution has a pH of 2.876?   A.…

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Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc…

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

Q: Write the Henderson-Hasselbalch equation for a solution of formic acid,HCO2H. What is the quotient…

A: Weak acids dissociate partially in an aqueous solution and the extent of the dissociation is…

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: Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the…

A: Note! As you have not mentioned any specific subpart that you want to be answered, so I am solving…

Q: Consider the weak acid CH;COOH (acetic acid). If a 0.048 M CH3COOH solution is 5.2% ionized,…

A: Given that  Concentration of Acetic acid    [CH3COOH] =       C= 0.048M . Acetic acid is a weak…

Q: Ascorbic acid (vitamin C, C6H8O6) is a cliprotic acid (Ka1= 6.8 x 10-5 and Ka2 = 2.7 x 10-12). What…

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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: When 0.040 moles of a weak monoprotic acid is dissolved in 500 ml of water, the pH is 3.0. What is…

A: First moles can be find out by mol/ volume (in L ).

Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11.  What is the…

A: Given, concentration of HIO = 0.785(M) The equilibrium of HIO in aqueous solution is,  HIO(aq)…

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: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

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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: What is the PH of a solution in which 15 mL of 0.01M NaOH has been to 25 mL of 0.01M benzoic acid…

A: Consider the reaction of NaOH with benzoic acid to form sodium benzoate is as follows;…

Q: Complete the K expression for the weak acid behavior represented by HCOOH(aq)H+(aq)+HCOO-(aq) and…

A: Complete the K expression for the weak acid behavior represented as given below.

Q: Ka for a 0.100 M methanoic acid solution whose pH is 2.37 is   4.2x10-3   8.7x10-3   1.8x10-4…

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Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (C;HgO;)? CH3O;(aq) +…

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Q: The dihydrogen phosphate ion, H2PO4 –, is an amphiprotic substance. (a) Write a balanced equation…

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Q: What is the pH of a solution that is 0.025M formic acid, HCHO2, and 0.018M sodium formate,…

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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.