Find the pH of each mixture of acids. 0.105 M in formic acid and 5.5×10−2 M in hypochlorous acid

Q: What is the pH of a solution that has H+ concentration equal to 5.5 x 10^-5 M?

A: Given Concentration of H+ = 5.5 x 10-5 M

Q: What is the pH of a solution with a hydroxide ion concentration of 10-2 M?

A: [OH-] = 10-2 M  pOH = - log [OH-] pOH = - log (10-2) = 2 At room temperature; pH + pOH = 14 pH + 2 =…

Q: A KOH solution has a concentration of 2.65 x 10-2 M. What is the pH of this solution

A:

Q: Acids have a pH between 0 and 6.9 and Bases have a pH between 7.1 and 14.  True  False

A: Find out given statement is true or false ?

Q: If a sample of a certain solution is determined to have a [H30+] concentration of 7.74×10-3…

A: We know that, pH is the negative logarithm of hydronium ion concentration. i.e.,…

Q: What is the pH of a solution that has a concentration of 2.0x10-5 M to 2 decimal places?

A: The PH of a solution can be calculated as follows

Q: What is the pH of 1.5 x 10-4M solution of H2SO4?

A: pH of a solution determines the concentration of hydrogen ion present in the solution.

Q: Find the pH of a 0.010 M HNO2 solution.

A: HNO2 is a weak acid with dissociation constant, Ka = 7.2 X 10-4  Hence HNO2 will dissociate…

Q: Which one is correct? What is the [H3O+] in a solution with pH=8? 10+8 M 10-8 M 8.0 M 6x10-8 M…

A: Given, pH = 8 PH is defined as negative logarithm of concentration of [H+] ion.

Q: What is the pH of a solution that is 2.7×10-9 M in NaOH

A:

Q: Determine the Kb of a weak base if a 0.19-M aqueous solution of the base at 25⁰C has a pH of 10.88

A: The question is based on the concept of equilibrium. we have been given a weak base  whose PH and…

Q: HClO is a weak acid (?a=4.0×10−8 M)and so the salt NaClO acts as a weak base. What is the pH of a…

A:

Q: What is the pH of a 6.50 x 10-5 M KOH solution? (This solution is also basic)

A: 6.50 × 10-5 M solution of potassium hydroxide releases 6.50 × 10-5 M hydroxide ion. The pOH is equal…

Q: Find the pH of a solution that is 9.0x10^-2 M in H2CO3

A: To calculate the pH we have to know the concentration of [H3O+]. As we know  pH= -log [H3O+] in the…

Q: Calculate the pH of pure water

A: Given :- Kw = 2.4 × 10-14  To calculate :- pH of pure water at 37°C

Q: Find the pH of a 0.0100 M sulfuric acid (H2SO4) solution

A: Given: Sulphuric acid (strong acid) Given acid is strong acid hence it completely dissociates into…

Q: basic solution is 7.60 × 10-12

A:

Q: What is the pH of 2.9x10 M

A:

Q: What is the pH of an HCl solution that has a concentration of 0.015 M?  Show your solution

A: pH can be defined as the hydrogen ion concentration present in solution that refersrefers to acidity…

Q: What is the pH of a solution that has an OH- ion concentration of 3.20 M?

A:

Q: Calculate the pH value of 0.5 M NaCl

A: There can be 4 type of combinations of salt:A salt formed when a strong acid combines with a strong…

Q: Determine the pH of each solutions 9. Calculate the pH of a solution if [H+] = 0.33 M. Is the…

A: pH = - log [H+] If the pH is less than 7, the solution is acidic If the pH is more than 7, it is…

Q: When a 0.061M aqueous solution of a certain acid is prepared, the acid is 2.1% dissociated.…

A: For a weak acid - WA   ⇔     W+     +      A- The reactants and products are in equilibrium. Since…

Q: What is the pH value of the solution formed by mixing equal volumes of a strong acid solution with a…

A:

Q: Calculate the pH of 0.002 M HCl.

A: The HCl is a strong electrolyte thus it completely ionized into its constituting ion, H+ and Cl- and…

Q: An aqueous solution contains 0.050 M HCl at 25.0 °C. What is the pH of the solution?

A: The pH of the solution can be calculated as follows -

Q: Calculate the pH of the acid or base with the given information. Given pH of 0.1 M ammonia…

A:

Q: at 0.125 M aqueous solution of a weak base is 9.2% ionized. what is the pH of the solution?

A: Given  Concentration (c) = 0.125 M Percentage ionization = 9.2 % pH = ?

Q: a Solution 1 has [H]=7.3x102 M, and solution 2 has [H]= 6.2x10 M. Calculate pH of both solutions. pH…

A: pH :-  The negative logarithm to the base 10 of  H+ ion concentration expressed in mol/L of an…

Q: Find the pH of a 0.72M hydrochloric acid solution

A:

Q: Using a graphical approach, solve for the pH of the following solution: 10-3 M (NH4)2CO3

A:

Q: Find the pH of the 4M NaH2AsO4 solution (Kai-5.8x10-³, Kaz=1.1x107)

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the given…

Q: What is the pH of a 0.021 M HCIO4 solution? Enter your answer in decimal format with two decimal…

A: If the given acid is a strong acid, then it ionises completely. For strong acids: pH =-log [H3O+]…

Q: Type your answers in all of the blanks and submit A What is the pH of an aqueous solution with [H*]…

A: pH is defined as the negetive logarithm of Hydrogen ion concentration. That is, pH = -log[H+]

Q: Find the pH of a solution with: [H+] = 1.6×10-6 M pH =

A: Given data, [H+] = 1.6×10-6 M

Q: Sodium hydroxide is a strong base. What is pH of a 0.02M sodium hydroxide solution?

A:

Q: What is the pH of a solution with a hydrogen-ion concentration of 1 x 10-4 M?

A:

Q: What is the pH of a 3.47 x 10 ^-4 M solution of hydrochloric acid?

A: Given data is as follows: The concentration of hydrochloric acid  = 3.47×10-4 M The pH of the…

Q: If a 0.030 M solution of a base has pH = 10.50, find Kb for the base.

A: Given data  pH=10.50 Concentration of solution = 0.030 M Suppose a weak base AOH then dissociation…

Q: Calculate the pH of a 7.4 x 10–4 M solution of Ba(OH)2.

A: We will Calculate pH.

Q: Complete the following table by finding (i) to (ix): [H'] [OH ] pH Acidic, Basic, Neutral? (1) (iv)…

A: In a solution, when concentration of H+ and OH- are equal then pH of the solution found to be 7 and…

Q: What is the pH of the solution? [OH-] = 8.4 x 10-3 M use significiant figures

A: pH is scale from which we determine either the given solution is acidic or basic. The pH scale is…

Q: A solution has [H*] = 2.5 x 10-9. What is the pH of the solution? [ Select] Is the solution acidic…

A:

Q: Determine the pH of the following solutions: 1.    [H+1] = 2.3 X 10-13 M   2.    [H+1] = 7.3 X…

A: Since you have posted a question with multiple subparts, we would answer only first three subparts.…

Q: Step by step please clearly

A: Given reaction,

Q: Calculate the pH of a solution that is 0.0718 M NaClO at 25°C

A: Given-> Molarity = 0.0718 M

Q: The pH of a weak base (B) is 9.99 when the concentration of the weak base is 0.18 M. What is the…

A:

Q: solution has a [H+] of 2.5 ×10-3 M.  What is the pH of this solution?

A:

Q: What is the pH of a 0.25 M solution of a strong acid?

A: The Formula of pH of solution is        pH = -log10[H+]

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.