Question 16 What is the pH of a 0.030 M LIOH solution? 1.52 12.48 3.00 11.00

Q: Question 8 Strong/Weak Acids A. Classify each of the following as a strong acid or a weak acid.…

A: Answer  Classify each of the following  Strong acid :- which is 100%…

Q: QUESTION 6 Calculate the pH of a solution that contains 3.9 x 10 MH30* at 25°C, 4.41 8.59 5.41 0.59…

A: Given, A solution contain concentration of [H3O+] is  3.9×10 -5 , the pH of the solution is:

Q: How many mL of 0.400 M KCI would be required to make a 0.0480 M solution of KCI when diluted to…

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Q: What is the approximate pH of a 0.5 M solution of NaOH? A O to 1 3 to 4 C 7 to 8 13 to 14

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Q: What is the pH of a 0.035 M aqueous solution of barium hydroxide? A) 12.85 B) 12.54 C) 1.46 D)…

A: Answer: pH basically represents power of hydrogen ion concentration in a solution. Its value is…

Q: What is the percent acid ionization in a 0.87 M weak acid solution with a pH of 2.30? 2.0% 87% 174%…

A: The objective of this question is to calculate the percent acid ionization in a 0.87 M weak acid…

Q: If the pOH of a solution is equal to 9.33, the pH of the solution is equal to 3.39. O True O False

A: Given  pOH of the solution = 9.33

Q: Find the pH of a solution whose [OH] is 2.8 x 10 5 M. O 2.8 O 9.4 O 4.6 O 13

A: Using relation between pH and pOH we can find pH.  Given [OH-] = 2.8 * 10-5M

Q: QUESTION 13 Which of the following acids is a weak acid?     HCl     HI     HBr     HF

A: The weak acids are those acids that are not able to release H+ in the solution. While the strong…

Q: Do you expect KClO4 ( OR "K" ClO4) to be acidic, neutral, or basic when dissolved in pure water?

A: The salts of strong bases and strong acids are neutrals at pH 7. The salts of weak bases and strong…

Q: Given that Kw for water is 2.4 x 10-14 at 37 °C, calculate the pH of a neutral aqueous solution at…

A: We are given Kw for water at 37°C equal to 2.4×10–14 . We need to calculate pH of neutral aqueous…

Q: Question 6 Which compound is the weakest acid? O Bicarbonate ion (HCO3) O Formic Acid (HCOOH) O…

A: Explanation :

Q: QUESTION 2 What is the pH of a 0.02 M solution of the strong base KOH? O 1.7 O 12.3 O 14.0 O 8.3

A: Conc. Of OH- =0.02M Find out PH

Q: QUESTION3 What is the pH of a 0.020 M HCIO4 solution? 12.30 1.70 0.040 0.020

A: The pH is amount  of H3O+  present in the solution .

Q: weakest acid?

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Q: Question 14 Calculate the pH of the resulting solution when 20.0 mL of 0.150 M NaOH is added to 50.0…

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Q: Calculate the pH of a solution that has [H301 = 3.1 × 10-8 M. A) pH 3.18 B) pH = 3.10 C) pH 7.51 pH…

A: Answer

Q: What is the pH of a 4.7 × 103 M HI solution?

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Q: The pH of a solution is 3.95. What is the OH¯ concentration in the solution?

A: The given problem can be solved by using the formula given below as; Given date: pH of the solution…

Q: Question 30 What is the pH of a solution that has an OH concentration equal to 2.9 x 102 M?

A: Given that : Concentration of OH- = 2.9 x 10-2 M We have to calculate the pH of the solution.

Q: QUESTION 19 Determine the pH of a 0.500 M NH3 solution at 25°C. The K, of NH3 is 1.76 x 103 O 10.281…

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Q: What is the pH of the solution if hydronium ion, H3O*, concentration is 3.0 x 10-9 M? Is the…

A: Given :- concentration of H3O+ i.e. [H3O+] = 3.0 × 10-9  To calculate :-  pH of solution  Nature of…

Q: An unknown weak acid with a concentration of 0.510 M has a pH of 5.600. What is the Ka of the weak…

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Q: QUESTION 2 Determine the pH of a 0.023 M HNO3 solution. 2.49 1.64 12.36 2.30 3.68

A: Given, The molarity of HNO3 is 0.023 M The pH of the solution is :

Q: What is the pH of a 0.015 M aqueous solution of barium hydroxide? A) 12.18 B) 12.35 C) 1.82 D)…

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Q: Question 6 Indicate whether the statement below is true or false. A solution with a pH of 2 has a…

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Q: The pH of an acidic solution is 5.53. What is [OH-]?

A: The pH of the solution is = 5.53We know that:

Q: ne pH of a 0.6 M

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Q: Of the following, ________ is a weak acid. A) HF B) HCl C) HBr D) HNO3 E) HClO4

A: Acidic strength of any acid is decided by the ability of acid to produce protons in the solution.…

Q: 14) Do you expect NaBr to be acidic, neutral, or basic when dissolved in pure water?   Question 14…

A: Acid base theory- Acids and bases have their own importance in chemistry. Acids and bases are…

Q: In the ionization of hydrofluoric acid with water,  _____ is the acid,  _____ is the conjugate base,…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: Question 1 Under what condition is the hydronium ion concentration in water expected to be zero? A…

A: Hydronium ion is a strong acid so  if it is present in strong base then it will react and form a…

Q: The pOH of a basic solution is 3.67. What is pH?

A:

Q: Question 5 An acidic solution contains _______ ions. K+, OH-, H+, Cl- A basic solution contains…

A: According to Arrhenius theory of acid and base  Acid is a substance that give H+ ion upon dissolving…

Q: QUESTION 19 What is the pH of a solution with H30* acid, base, or neutral. = 0.00743 M? Give the…

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Q: Question 3 What happens to the pH value as the concentration of OH increases? O It decreases O It…

A: pH is a scale used to measure acidity or basicity of an aqueous solution.

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.