Given the pOH for a solution, calculate the other values:   pOH = 5.33   a)   pH =  b)   [H3O+] = ? X10^?  c)   [OH-] =? X 10^?  d)   acidic, basic, or neutral?

Q: The pH of an orange juice is 3.33, calculate its [H+] and [OH-]

A: We can determine the hydronium and hydroxide ion concentration by applying the formula of pH =…

Q: A) In the lab, you're working with a solution and measure it's pH with a meter to be 6.9. However,…

A: We know that, pH is the negative logarithm of hydronium ion concentration and pOH is the negative…

Q: A sample of saliva has a pH of 5.8 Which statement describing the saliva sample is NOT true?   (a)…

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Q: Calculate the pH of a 0.094 M Ba(OH)2 solution. pH =

A: pH is determined by knowing the concentration of H+ ion in solution . Mathematically it is…

Q: If a solution has a [OH-] = 2.551 x 10-2 M, what is the pH of the solution?   Determine the [H3O+]…

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Q: The pOH of an acidic solution is 8.87. What is [H*]?

A: We know that, the sum of pH and pOH is equal to 14.i.e.                            pH + pOH = 14…

Q: Calculate [OH -] and pH for each of the following solutions.(a) 0.0071 M CsOHOH- = ____ pH = _______…

A: Hey, since there are multiple sub-part questions posted, we will answer first three questions. If…

Q: [H;O'] [OH'] pH pOH acidic or basic ? 1.7 X 10:1ºM 8.79

A: pH = -log[H+] pOH = -log[OH-] pH+pOH = 14 If pH>7, basic If pH<7, acidic

Q: Calculate [OH-] for a solution with a pOH of 8.03. What is the[H3O+] of this solution? What is the…

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Q: What is the [OH-] of this solution?

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

Q: What is the pH of a bleach solution that has a [OH−]=7.1×10−4 M?[OH−]=7.1×10−4 M? pH=pH=     Is…

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Q: 6. Calculate the pH of the solution if the concentration of [H3O] ion is 2.0x10 M at 25°C.

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Q: QUESTION 6 If an aqueous solution has a hydronium ion concentration of B.2 x 10* M, (a) what is the…

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Q: (a) blood, pH = 7.50 acidic Obasic neutral (b) gastric juice, pH = 2.50 acidic Obasic M neutral M

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Q: Aspirin, which is acetylsalicylic acid, was the first NSAID use to alleviate pain and fever. If a…

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Q: Calculate the pOH of a solution that has [OH-] = 3.6 x 10 -5 M

A: pOH of any solution is given by  pOH = -log[OH- ]  where [OH- ] = concentration of OH- ions in M

Q: The normal pH of blood is 7.4. What is the [H+] of normal blood? Is it acidic, basic, or neutral?

A: Answer :-  a) The [H+] of normal blood = 4.0 × 10-8 (M)  b) The nature of Normal Blood = Basic…

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 3.47? (b) What are [H₃O⁺],…

A: pH is equal to the negative logarithm of hydronium while pOH is equal to the negative logarithm of…

Q: If HNO3 is added to water, how does [OH-] change? How does pH change? (b) Use the pH…

A: a. HNO3 releases  H+ in the water Therefore, acidity of water increases pH of water decreases HNO3 +…

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 8.97? (b) What are [H₃O⁺], [OH⁻],…

A: The concentration of the hydrogen ions in the solution is determined in the pH scale.…

Q: Determine the H30* concentration in the following solutions. Identify each solution as acidic,…

A: If the pH>7: Basic solution If pH < 7: Acidic solution If pH =7: Neutral solution (a) pH…

Q: An aqueous solution is found to have an OH- concentration ( [OH-] ) of 1.0 x 10-8 M, a) What is the…

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

Q: iii)[OH−] = 5.1 × 10−7 M

A: 4) a) The autoionization of water is -             2H2O (l) ⇌H3O+ (aq) + OH- (aq)  The equilibrium…

Q: 6. A substance has a [H,O'] of 5.21 x 10³, determine [OH], pH and pOH and determine if the substance…

A: [H3O+][OH-] = 1 x 10-14 pH = -log[H3O+] pOH = -log[OH-] pH < 7 , acidic pH > 7 , basic pH = 7,…

Q: The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per…

A: pH of solution is defined as negative logarithm of hydrogen ions  present in solution.

Q: 1.Why does the autoionization of water occur? 2.What is the definition of a strong acid? The…

A: Note - Since you have posted a question with multiple sub-parts, we will solve the first three…

Q: The pOH of an acidic solution is 8.53. What is [H⁺]?

A: Answer: [H+] = 3.4 ×10-6 M

Q: The pOH of an acidic solution is 8.81. What is [H⁺]?

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Q: The autoionization constant for water at 35 °C is 2.2 × 10−14. Use this information to answer the…

A: " Since you have posted a question with multiple sub-parts , we will solve first three sub-parts for…

Q: A solution has [H3O+] = 1.20 x 10-4 M. What is the pH of the solution?

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.