(1point) Calculate the pH and pOH of a 4.3 x 10 M solution of NaOH.

Q: The pOH of an aqueous solution of 0.591 M caffeine (a weak base with the formula C3H10N,02) is

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Q: The weak acid, HA, has a Ka of 1.60 x 10-10. What is the Kb of its conjugate base, A™?

A: Given :-  Ka for weak acid (HA) = 1.60 × 10-10  To determine :  Kb of its conjugate base (A-)

Q: dissociated H+H+ ions

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Q: 3. Which of the following is a more concentrated acid 0.01 M HNO3 or 1.0 x 10+M HNO3. Does each…

A: A concentrated acid contains a large amount of acid in a given volume whereas a dilute acid contains…

Q: (d) Do you expect the pH of the pure water at 100 °C will be 7, lower than 7, or higher than 7? Give…

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Q: What is the pH of 0.00083 M CsOH? Is the solution neutral, acidic, or basic?

A: Given; Concentration of caesium hydroxide solution, [CsOH] = 0.00083 M pH of the caesium hydroxide,…

Q: What is the pH of 3.78 *10^-2 M nitric acid in aqueous solution ?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

Q: what is the pH of a 3.25x10^-4M solution of H+?

A:

Q: A tablet containing 500 mg of aspirin was dissolved in enough water to make 100 mL of solution.…

A: Given, Mass of aspirin, C9H8O4 = 500 mg = 0.500 g     (1 mg = 0.001 g) Volume of solution = 100 mL =…

Q: The value of Ka for phenol (a weak acid) is 1.00×10-10. What is the value of Kb, for its conjugate…

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Q: 1. Which is the pH of 1M NaOH solution?

A: The answer for the first question is given below. Kindly repost the other questions as separate…

Q: The value of Ka for hypochlorous acid is 3.50x10-8. What is the value of Kb, for its conjugate base,…

A: The dissociation of the hypochlorous acid takes place as follows: HClO + H2O  → H3O+ +  ClO-

Q: The pOH of ammonium hydroxide at 25 C is 5.55. What is the pH and the [H ], [OH ] in mol/L for…

A: At constant temperature, the pH of a solution remains constant. For 250 C, the pH of the solution…

Q: What is the pH of the solution obtained when 130 mL of 0.610 M NaOH is diluted to 16.0 L with water?…

A: Given: Initial concentration of NaOH = 0.610 M Initial volume of solution = 130 mL = 0.130 L…

Q: For a given aqueous solution if [H+]=7.92x10-5M, what is [OH-]

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Q: What is the pOH of a solution with a pH of 2.5?

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Q: If H+ is equal to 6.9×10^-5, what are the values of pH, pOH, and OH-?

A: Given: [H+]=6.9×10-5 To find: pH, pOH and [OH-]

Q: What is the pH of a solution that is 1 × 10-8 M with respect to H+?

A: Here given, Concentration of H+, that is [H+] = 1 x 10-8 M We know, that---- PH = - log [H+]

Q: When the pH is 7, there is no H30* or OH in solution.

A: A question based on pH concept, which is to be accomplished.

Q: In an aqueous solution at 25 C, if [H3O+]=3.1×10^-4M, then [OH-] is

A: Given data: The hydronium ion concentration is H3O+=3.1×10-4 M. To find: The hydroxide ion…

Q: 1--The solution of substance (X) is completely ionized in water, its pH value is (10), so its…

A: Dear student , since you have posted multiple questions we are allowed  to solve only first question…

Q: pH

A:

Q: 4. Calculate either [H3O*] or [OH-] for each of the solutions at 25 °C.

A: 4)  As we know,   pH + pOH = 14  And [OH-][H3O+] = 1.0×10-14 Solution A. [OH-] = 2.15×10-7 M  [H3O+]…

Q: 6. [H*] for = 1.57x10 M, what is the [OH]?

A: pH is quantitative measure of the acidity or basicity of aqueous  solutions. This is widely used in…

Q: What is the pH of a 3.9×10-2 M solution of KOH at 25 °C?

A: KOH ionizes in aqueous solution as,                          KOH (aq)       -----> K+ (aq)   +…

Q: Determine the [H+][H+] , pH, and pOH of a solution with an [OH−] of  0.099 M at 25 °C.

A: The concentration of hydrogen ion is calculated as follows:

Q: Determine the (a) degree of ionization and (b) percent ionization of ethylamine, C2H5NH2 in an 0.85…

A: Given concentration of ethylamine = 0.85 M Standard value Kb for ethylamine = 4.3*10-4

Q: How much NaOH (in grams) is needed to prepare 546 mL of solution with a pH of 10.00?

A: ANSWER IS :

Q: Given that for water at 37 °C Kw = 2.4x10 1 what is the pH of a neutral aqueous solution at 37 °C?…

A: for water , Kw = [H+] [OH-]   pH of water depends on temperature.

Q: Calculate [H30*] of a solution with a pH of 5.5

A: Given information: pH of solution = 5.5

Q: What is the pH of a 10-¹⁰M NaOH solution?

A:

Q: At the freezing point of water (0 °C), Kw = 1.2 x 10-15.Calculate [H+] and [OH-] for a neutral…

A: Water can undergoes auto-ionization to form H3O+ and OH- ions. In neutral solution, [H3O+]=[OH-]…

Q: To what volume should you dilute 1 L of a solution of a weak acid HA to reduce the [H+] to one-half…

A: Break down the compound.  [HA]→ [H3O+][A-].  Ka is constant for any given [HA]. Reduce  [H3O+] to…

Q: The pOH of a 0.07 M NgOH solution at 25 °C is:

A: Given :- concentration of NaOH = 0.07 M  To calculate :- pOH of the solution

Q: Q1. Identify if the solution on the left is a strong or weak acid or base. Explain in detail how you…

A: The reaction taking place is given as,

Q: How much NaOH (in grams) is needed to prepare 584ml of solution with a pH of 12.00?

A: Since NaOH is a strong base  Hence it will dissociate completely into ions forming Na+ and OH- ions…

Q: The ka of an acid is 7.6 times 10-3 at 25 degrees celsius, what is the kb of the conjugate base?

A: The ionic product of water is equal to the product of dissociation constant of conjugate base and…

Q: What is the pH of a 0.0380 M solution of HONH,CI (Ka of HONH,+ is 9.1 × 10-7)?

A:

Q: Determine the pHpH for the following solutions: A) [H3O+]=7.7×10−2M[H3O+]=7.7×10−2M, Express your…

A: pH is a negative logarithm of Hydrogen ion concentration. It is given by Sorenson. It can be written…

Q: An aqueous solution at 25°C has a pOH of 6.6. Calculate the pH. Round answer to 1 decimal places

A: From given data,  pOH = 6.6    Also, at 25°C,  pOH + pH = 14..............equation 1

Q: Calaiste t PH and the POH FOR a 06 M Solution of Ca(OH)₂

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Q: An aqueous solution at 25 °C has a pOH of 4.28. Calculate the pH. Round your answer to 2 decimal…

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Q: Q 2. Identify if the solution on the left is a strong or weak acid or base. Explain in detail how…

A: The solution has a pH of 3.05. pH between 0 to 6.9 is for acid. pH between 7.1 to 14 is for base.

Q: What is the pOH of a 0.00502 molar HCl solution at 25 °C?

A: Hydrogen chloride is a strong acid that dissociates completely in aqueous solution.

Q: What is the pH of a 6.50x10^-3 M KOH solution?

A:

Q: The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the…

A: Since for any acid and its conjugate base, the Ka and Kb respectively are related to each other as…

Q: 5) What is the pH and pOH of a solution with a [H,0'] of 5.72X 10* M? Is the solution acidic, basic…

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

Q: Calculate [OH−] for the following solution; [H3O+] = 8.87×10−9 M Is the solution basic at 25°C?

A: pH is negative logarithm of hydronium ion. Given,  [H3O+] = 8.87×10−9 M

Q: What's the pH of a solution with an H+ concentration of: 1.247 x 1012, Round to 2 decimal places.

A: Value of pH is used to measure the acidity or basicity of a solution. At room temperature, value of…

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.