Determine the hydroxide ion concentration in an aqueous solution of HBr with pH = 3.98 at 25 °C. 5.6x1010 M 1.0x1014 M 9.5x10-11 M 1.0x10-7 M 1.8x10-5 M

Q: Determine the pH of the molecules given in a 1L beaker containing 0.035M solution of the given…

A: Given,  The molarity of each solution in 1 L beaker is 0.035 M.  The pH of the solution is:

Q: Refer to the following ionization of hypochlorous acid: HOCI (aq) + H₂O (1) H3O+ (aq) + OCI (aq) 1…

A: Given reaction: HOCl(aq) + H2O(l) ⇌ H3O+ (aq) + OCl-(aq) The Ka for HOCl = 3.5×10-8 The initial…

Q: What is the pH of a 0.200 M solution of HNO3? A 0.70 B 1.31 c) 6.18 (D) 8.53

A: Given, the concentration of HNO3 =0.200 Mwe are asked to calculate the pH of solution of HNO3

Q: Calculate the pH and pOH of each solution at 25 °C. a. [H30'] = 1.7 x 10M c. [H,O'] = 2.2 x 106M b.…

A: Given,

Q: What is the pH of a 2.3 x 10-3 M LIOH solution? O 11.4 O 2.82 O 2.64 O 11.2

A:

Q: Calculate the pH and pOH for each of the solutions with the following hydrogen ion or hydroxide ion…

A: pH is is defined as power of hydrogen  PH = log [H+]

Q: Calculate the pH and pOH for each of the following solutions: Solution pH pOH 2.5 M OH–

A:

Q: 9. Which of the following solutions for a weak acid at equilibrium would have the largest pH? b. 3.2…

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

Q: Calculate the pH of a 0.36M methylamine (CH3NH2) solution, if Kb = 4.4x10-4

A: Solution- methylamine (CH3NH2)  is weak base which ionisation is as follow; CH3NH2+H2O→CH3NH3++OH-…

Q: For the reaction of hydrazine (N2H4) in water, H,NNH, (ag) + H20(1) H,NNH3+ (ag) + OH (ag) K, is 3.0…

A: The given equilibrium reaction is as follows, H2NNH2(aq) + H2O(l) ↔H2NNH3+(aq) + OH-(aq) The…

Q: What is the pH of a 1.40*10^ -2 mol/L Ca(OH)2 solution? (NOTE: To determine the actual hydroxide…

A: Given : Concentration of Ca(OH)2 = 1.40 X 10-2 mol/L

Q: What is the pH of a 0.010 M solution of aqueous Sr(OH)2?   a. 10.2   b. 2.0   c. 9.0   d.…

A: To determine the pH of a basic solution, the pOH is determined first and then pH is calculated using…

Q: 9. Which of the following solutions for a weak acid at equilibrium would have the largest pH? d. 3.2…

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

Q: Calculate the pH value in each of the following solutions given their [H3O+] concentration.…

A: Given;

Q: What is the pH of a solution with the hydroxide ion concentration [OH] = 5.67 x 1C %3D O 3.25 O 4.00…

A: Given, OH- = 5.67 × 10-4  we know, => pOH = -log[OH-] => pOH = -log(5.67 × 10-4 ) => pOH =…

Q: What is the pH of .15 M KBRO(aq)? O 3.07 O 4.75 O 13.18 O 9.25 O 10.93

A:

Q: The pH of a 0.045 M Ca(OH)2 solution is: +1.3467 O +12.954 O +12.653 O -1.3467

A:

Q: Determine the pH and [OH-] concentration of a 2.56 x 10-4 M HNO3 solution.

A: pH = -log [H+] pOH = 14 - pH [OH-] = 10^-pOH

Q: What is the pH of 5.35 x 103 M H2CO3 (aq)? O 4.3 O 8.6 O 2.3 O 4.9 O 9.1

A: Concentration of H2CO3 = 5.35 × 10-3 M  pH of the H2CO3 = ?

Q: What is the pOH of a 0.030 M solution of barium hydroxide? A)12.78 B) 12.48 C) 1.52 D) 1.22 E)…

A: Given  0.030 M solution of barium hydroxide

Q: What is the the PH and POH of the following solutions: 1. 0.05 M Ba(NO3)2 2. 0.01 M Na2SO4

A: The given solutions are 0.05 M Ba(NO3)2 and 0.01 Na2SO4.

Q: Determine the pH of each of the following solutions. (a) 0.684 M hypochlorous acid (weak acid…

A:

Q: %. What is the pH of 0.0015 M solution of nitric acid? a. 1.41 c. 5.65 b. 2.82 d. IL.18

A: To calculate the pH of 0.0015 M solution of nitric acid.

Q: Calculate [OH ]in an aqueous solution with a pH of 4.33 at 25°C. 6.3 x 10 6 O 3.8 x 10-5 O 2.1 x 10…

A: [19.]  pH = 4.33 (given)  [H+] = 10-pH  [H+] = 10-4.33  [H+] = 4.677 × 10-5 M Hence, [OH-] = 10-14 /…

Q: Calculate the pH of a 0.052 M (C2H5)2NH solution (Kh = 1.3 × 10). pH =

A:

Q: The pH of a 0.100 M CH3NH2 solution is 11.80. What is the % ionization value? O 11.80% O 1.58% O…

A:

Q: Calculate the pH of a 5.7 x 10 M aqueous solution of hydrobromic acid (HBr). -5

A: Given :- concentration of HBr solution = 5.7 × 10-5 M  To calculate :- pH of solution  pH =…

Q: 1 You are presented with a solution that has a pOH of 2.13,What is the pH of this solution? O 11.87…

A: The pOH of the solution is = 2.13 The pH of the solution is =?

Q: Calculate both the pH and pOH for each of the solutions with the following hydrogen ion or hydroxide…

A:

Q: For the reaction of hydrazine (N2H4) in water, H,NNH, (ag) + H20(1) = H,NNH3* (aq) + OH (ag) K, is…

A:

Q: Calculate the pH of a solution in which the molar concentration of H+ is 1.6 x 10-9. a. 1.60 b.…

A: Given information,     Molar concentration of H+ is 1.6 x 10-9.

Q: Calculate the pH and pOH for each of the solutions with the following hydrogen ion or hydroxide ion…

A: The equations which we relate pH and pOH are  pH + pOH = 14 And the pH and pOH of any solution is…

Q: What is the pH of a 8.82 x 10-2 M solution of NaOH? O 12.9 O 10.9 O 6.91 09.90 O 1.05

A:

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)…

A:

Q: What is the pH of 2.7 x 102 M NaOH(aq)? O 3.6 O 1.6 Ο 12.4 O 13.1 O 10.4

A:

Q: Determine pH of a 0.12 M ammonia solution.

A: Base dissociation constant Kbis utilized to determine the basic nature of a solution. It refers to…

Q: Determine the pH of 0.25M CH3COONA solution. Kg of CH3COOH = 1.8×105 Select one: 10.08 O 9.08 O 4.90…

A: Sodium acetate is a salt of a weak acid, acetic acid, and strong base, sodium hydroxide. The salt of…

Q: what is the ph of a 0.81 M hypochlorous acid (HClO) solution?

A: Given :- concentration of HClO = 0.81 M                 Ka = 3.0 × 10-8  To calculate :- pH of…

Q: Determine the pH of the solution resulting from mixing a solution of 154 mL of HNO2 (Ka = 5.62e –…

A:

Q: Calculate the pH of a 3.5 x 10-3 M HNO3 solution.

A: Nitric acid HNO3 is a strong acid. Hence, it completely dissociates in the aqueous solution.

Q: For Ni(s) 2H* (? M) H2 (1 atm) Ni*2 (1 M) E = .01v + Calculate the pH of the solution.

A:

Q: An increase in the H* concentration by a factor of 1000 implies which of the following? A) The pH…

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

Q: What is the pH of a 0.010 M solution of HF?(a) 1.58 (b) 2.10 (c) 2.30 (d) 2.58 (e) 2.64

A: HF is a weak acid with dissociation constant Ka = 6.8 X 10-4 The dissociation reaction of HF is  HF…

Q: Find the pH and the pOH of the solutions 1. A 0.023 M solution of hydrochloric acid   2. A 6.6 x…

A:

Q: What is the pH of a 0.025M solution of sulfuric acid? Ka₂ = 1.2 x 10-² pH = [?]

A:

Q: What is the pH of a 1.25 M solution of HCIO? HCIO (aq) + H20 (1) = H3O* (aq) + CIO (aq) Ka =2.88 x…

A:

Q: Which of the following .1M acid solutions will have the lowest pH? A. HIO3 B. HCLO3 C. HBRO3 D.…

A: Strongest acid has lowest value of pH.

Q: Finding pH The hydrogen ion concentration of a sample of each substance is given. Calculate the pH…

A: (a) Lemon juice [H+] = 5.0 × 10-3M (b) Tomato juice [H+] = 3.2 × 10-4M (c) Seawater [H+] = 5.0 ×…

Q: Calculate the pH and molar concentration of H+ for the following strong acid and base: a) 1.318 M…

A:

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.