What is the pH of a 9.27*105 M solution of H3O? O 4.03 O 9.97 O 12.81 O 2.98

Q: If pH of a solution of NaOH is 12.3, then what is the value of [H+] ? O 12.3 M O 5.01x10-13 M O 5.01…

A: Given that the pH of a solution of NaOH is 12.3. To calculate the [H+] of the given solution.

Q: Calculate the pH of a 3.5 × 10–3 M HNO3 solution.

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

Q: Calculate the pH of a 0.48M HNO3 solution.

A: Concentration of HNO3 solution = 0.48 MpH of the solution = ?Note: pH can be define as the negative…

Q: What is the pH of a 0.25 M solution of NH3? Kb = 1.8x105 O 2.67 O 11.33 O 9.07 O 4.93

A: Given valuues from  the question, Salt concentration = c= 0.25 M Kb =1.8×10--5 then,

Q: What is the pOH of a solution that has a pH of 2? O 12 7 O 14 O 16

A: Given , pH of the solution is 2. pH and pOH measures how acidic or basic is the solution is.

Q: Calculate the pH of a 0.307 M NH3 solution. NH3 has a ?b=1.8×10−5.

A: First of all a balanced reaction should be written for the solution: Here, water concentration is…

Q: What is the pH of a 7.7 × 10⁻⁴ M HClO₄ solution?

A: The HClO4 is a strong acid and it fully dissociates in water as H+ and ClO4- So the concentration of…

Q: Calculate the pH of a solution with [H+] = 3.7 x 10-5 M O 5.00 3.76 O 9.67 O 4.43 O 12.5

A:

Q: Calculate the pH of a 2.4 x 105 M HBr solution at 25 °C. O 2.45 O 11.69 O 4.62 O 9.38

A:

Q: What is the pH of a 0.0040 M Sr(OH)2 solution? O 12.00 O 2.40 O 11.60 O 11.90 O 2.10

A: Strong acids or bases  are dissociated completely. so we can direct calculate its [H+] or  [OH-]…

Q: Calculate the pH of a 0.0348 M HNO3 solution.

A: We have to find pH of given acid

Q: Calculate the pH of a 0.0015 M solution of C6H5NH2 (Kb for C6H5NH2= 3.80 x %3D

A: given :- concentration of C6H5NH2 = 0.0015 M  Kb for C6H5NH2 = 3.80 × 10-10  To calculate :-  pH of…

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 3.1 x 105M HBr solution? O 4.09 O 4.51 O 8.1 O -4.09

A:

Q: pH

A:

Q: What is the pH of a 0.605 M solution of HNO₃?

A: The given data is as follows: The concentration of HNO3 = 0.605 M The pH of HNO3 solution = ? The pH…

Q: The pH of a 0.02 M NgOH solution at 25 °C is: O 12.8 O 13.7 O 1 1.5 O 12.3 O 13.1

A:

Q: How does the hydronium ion concentration, (H3O+) change when the pH of a solution is lowered from…

A: pH = -log[H3O+]  log[H3O+] = -pH  so, [H3O+] = 10-pH

Q: What is the pH of a 3.00 x 10−8 M solution of HClO4? 6.48 7.00 6.89 7.52 7.15

A: Applying formula  pH = - log[H+] = -log[H3O+]  Equation  HClO4(aq) ———>  H+(aq)  +  ClO4-(aq)

Q: What is the pOH of a 0.033 MHNO3 solution? O 10.59 1.48 3.41 12.52 15.48 14

A:

Q: What is the pH of .03 M HC2H3O2 (aq)? O 10.07 O 1.52 O 4.74 O 3.13 O 6.27

A: Ka is acid dissociation constant which determines strength of acid. Stronger acid dissociates more…

Q: : What is the pH of a 0.400 M HNO O 0.40 O 2.05 O 0.60 O 4.12 O 1.67

A: HNO3 when dissolved in water it dissociates.

Q: Which of the following pH values would indicate a basic solution? 04 0 7 O 10 O 3

A: The answer to the following question is given as:

Q: What is the pH of a 1.45 X 10-6 M solution of HNO3?

A: We have given that   Concentration of HNO3 = 1.45×10-6M  We know that  HNO3 is strong acid and…

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: 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: What is the pH of a 0.395 M HNO3 solution?

A: pH can be calculated using the formula: pH = - log[H3O+] = - log[H+]

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 13.8 O 13.1 O 1.5 • 12.7 O 10.3

A:

Q: What is the pH of wine that has an H 3O + concentration of 3.2 × 10 −4 M?

A: The pH scale is used to measure the acidity and basicity of aqueous solutions. pH is the negative…

Q: What is the pH of a 0.20 M NaBrO2 solution? Ka for HBRO2 =1.2 x 10 O 11.39 O 3.45 O 9.11 O 8.76 O…

A:

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 10.3 O 12.7 O 11.5 O 13.1 O13.8

A: pH of solution is calculated using relation pH + pOH = 14

Q: Calculate the pH of a 0.125 M HNO3 solution.

A: Working formula pH = -log[H+]

Q: What is the pH of a 0.031 M solution of aqueous Sr(OH)2? O 1.21 O 1.51 O 12.49 O 12.79

A: pH of an aqueous solution is defined as the negative logarithm of H3O+ ion concentration.…

Q: The pH of 0.075 M NH3 solution (Kb for NH3 = 1.75 × 10-5) O 4.94 O 12.03 O 1 1.05 O 8.02 O 2.09

A: Given,  Concentration of NH3 = [NH3] = 0.075 M  Base dissociation constant of NH3 = Kb = 1.75 x 10-5…

Q: 1. Which acid would produce the salt Zn(NO3)2? O HNO3 О нс O H+ Он HI

A:

Q: What is the theoretical pH of a 0.000001 M NaOH solution?

A:

Q: What is the pH of a 0.200 M solution of HNO3?   0.70   1.31   6.18   8.53

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.