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

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 0.00349 M solution of HCl?

A: HCl is a strong, monobasic acid and dissociates completely as per the following reaction:- HCl (aq)…

Q: The pH of an acidic solution is 5.67. What is [OH⁻]?

A: Given:   pH of an acidic solution = 5.67  [OH-]= ?

Q: The pH of an acidic solution is 2.19. What is [OH]?

A: The question is best on the concepts of PH. we have to calculate hydroxide Ion concentration.

Q: If the pH of a solution is 1.78, what is the concentration of [H+]?

A: pH = -log [H+]

Q: The pH of an acidic solution is 3.67. What is [H⁺]?

A:

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−], of 1.35×10−8 M.

A:

Q: What is the pH of a 0.845 M solution of KOH?

A:

Q: The pH of a basic solution is 9.93. What is [OH ]?

A:

Q: What is the hydroxide ion concentration in a solution that has a pH value of 9.776?

A: Given, pH = 9.776  Concentration of the hydroxide ion = [OH-] = ? The formula used here are, pH +…

Q: Since the pH value of a solution is 9.67, what is the hydrogen ion concentration in that solution?

A: pH is the indication of potential of protons in a given solution and is the negative logarithm of…

Q: Calculate the OH- concentration for a solution with a pH of 3.66

A: Since pH = 14 + log[OH- ]  where [OH- ] = concentration of OH-  ion

Q: If the OH- ion concentration of a blood sample is 4.7 ×10−7 M, what is the pH of the blood sample?

A: We know that, pOH can be expressed as the negative logarithm of hydroxide ion concentration, i.e.…

Q: if the ph of a solution is 3.80, what is its hydrogen ion concentration?

A: Given:PH = 3.80.

Q: The pH of a basic solution is 10.59. What is pOH?

A: The sum of pH and pOH for a solution is equal to 14. pH + pOH = 14 Given that,pH = 10.59

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=1.6×10^−4 M?   pH=

A: The pH of an aqueous solution can be calculated using equation (1). In this equation [H+] represents…

Q: The pH of an acidic solution is 5.05. What is [OH^-]

A:

Q: If a solution has a proton concentration of 0.00156 M, what is the pH?

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: A sample of TANG juice has a hydronium-ion concentration of 1.7 x 10^-4 M. What is the pH? Is the…

A:

Q: What is H3O+ ion concentration of a solution that has an OH- ion concentration of 2x10-3 M?

A:

Q: The pH of a basic solution is 10.89. What is [H*]?

A: The pH of any solution is given by  pH = -log[H+] where [H+] = concentration of H+ ions in the…

Q: What is the concentration of hydronium ion in a solution if its pH is 4.80?

A: • The values provided in the question are:-    i) pH of a solution = 4.80    • We need to calculate…

Q: The pH of a basic solution is 12.83. What is [OH ]?

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

Q: The pH of an acidic solution is 5.79. What is [OH⁻]?

A: Given: pH = 5.79 [ OH- ] =?

Q: The pH of a solution is 6.88. Find the H + and OH- concentrations and pOH

A: pH is a scale used to determine the H+ ion concentration of a solution. pH is numerically negative…

Q: If the pH of a solution is 1.50, what is the concentration of [H+]?

A: pH of a solution is 1.50 We have to find the  concentration of [H+] We know that  pH = - log [H+]

Q: The pH of a basic solution is 12.59. What is [OH⁻]?

A: Given: The pH of a basic solution is 12.59 [OH-] is the concentration of hydroxide ion

Q: The pH of a solution is 5.330. The [OH-] is [concentration]

A: Given information,        pH of the solution = 5.330

Q: The hydronium-ion concentration of a solution is 8.6 × 10-6 M. What is the solution pH?

A:

Q: The pH of an acidic solution is 4.77. What is [OH⁻]?

A: According to theory of acid-base: pH + pOH = 14

Q: The pH of an acidic solution is 2.35. What is [OH-]?

A: Given that  The pH of an acidic solution; pH = 2.35. The concentration of OH- ion, [OH-]=

Q: What is the relationship between H+ and OH- concentrations in a solution that has a pH of 11?

A:

Q: What is the pH of a solution with a hydroxyl ion (OH−) concentration of 10−12 M

A: The pH of a solution with a hydroxyl ion (OH−) concentration of 10−12 M is to be calculated

Q: What is the concentration of hydroxide ion in a solution with a pH of 3.767?

A: pH of a solution is determined from the concentration of H+ ion in solution.  Now, pH = -log[H+]…

Q: Define pH of a solution. Calculate the pH of a 1.37M solution of HCI.

A: pH is the negative logarithm of concentration of H+ ions  pOH is the negative logarithm of…

Q: An aqueous solution has a hydroxide ion concentration of 5.0 x 10 8 M. What is the pH of this…

A: Given [OH-] = 5 × 10-8 M

Q: What is the pOH of a solution with a pH of 3?

A: pH of solution = 3pOH = To be determined

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

A:

Q: The pH of an acidic solution is 6.75. What is pOH?

A:

Q: A solution has a hydrogen ion concentration of 1 x 10^6 M. What is the pH?

A: The negative logarithm of concentration of hydrogen ion is known as pH. pH = – log [H+]

Q: If an aqueous solution has a hydrogen ion concentration of 1×10−2 M,1×10−2 M, what is the…

A: [H+] = 1 × 10-2 M We need to determine [OH-] .

Q: The pH of an acidic solution is 4.37. What is [OH]?

A:

Q: What is the hydrogen ion concentration of a solution with a pH of 2.0?

A:

Q: What is the [OH-] concentration of a solution with a pH of 3?

A:

Q: If a solution has an OH- concentration of 0.00135, what is the pH?

A: For the given solution the hydroxide ion concentration is given. Hence first of all we calculate the…

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−][OH−], of 7.69×10−7 M.

A: Calculate the pOH of the solution,            pOH =- log [OH-]= - log (7.69 × 10-7)= 6.11

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

A:

Q: The pH of a solution is 4.00. What is the hydroxide (OH-) ion concentration?

A: We know, pH=-log[H+]

Q: The pH of a solution is 3.10. What is the OH- concentration in the solution?

A:

Q: What is the difference between a strong and a weak acid?

A: Here we are asked to write the difference between the strong acid and weak acid.

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.