Find the pOH of a solution whose pH is 8. Answer:

Q: At 10.ºC, Kw = 1.14 x 10-15. What is the pH of water at 10.ºC? Choose the closest answer. 3.98…

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Q: find OH-(M) ph=2

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Q: Which acid is the most commonly produced acid and is used in large quantities in the petroleum and…

A: The correct answers of the above questions are given in following steps with proper reasoning.

Q: What is the pH of a 0.430 M HNO3 solution? Your Answer: Answer

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Q: In an aqueous solution of a certain acid with pK, = 3.24 the pH is 2.41. Calculate the percent of…

A: Assuming the acid given  is monoprotic acid HA. hence the dissociation reaction for the acid is  HA…

Q: Using the Kb from the previous question, what is the pH of an 0.0100 M solution of sodium benzoate.…

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Q: Determine the pH of a 0.420 M NH3 solution. The Kb of NH3 is 1.76 × 10-5. Enter the result to 2…

A: Concentration of NH3 = 0.420 M Kb of NH3 is 1.76×10-5  Now hydrolysis reaction of NH3 is given by…

Q: 4. Calculate the pH of a 0.47 M solution of HOI. (Ka= 2.3 x 10-11). Use 2 decimal places in your…

A: 4. For weak acid, pH = 1/2 pKa- 1/2 Log C

Q: . H+= 1.10^-1 = PH   2.) Ph=4.93 = [H+]

A: Given here two questions as follows, 1 [H+] =1*10-1 we are asked to calculate the pH of solution. 2)…

Q: Pre-lab question #9: If the PH of a solution is 6, what are the hydroxide ion concentrations?…

A: pH of a solution measures the acidity of the solution. If pH >7 solution is basic. If pH<7…

Q: Why is the color violet/blue at pH near 7? Answer in 1 sentence.

A: Answer -   The colours from yellow to red indicate an acidic solution, colours blue to violet…

Q: 5. Which one of these molecules would you expect to be the stronger base? Justify your answer. N.

A: For the given nitrogen containing compounds in the question, localization of the lone pair of…

Q: Calculate the pH of a 0.0076 M solution of acetic acid, CH3COOH. The Ka of acetiç acid = 1.8 x 10-5.…

A: Kaa of acetic acid = 1.8× 10- 5  initial concentration of acetic acid = 0.0076 M

Q: if hydronium ion concentration= 4,5•10^-9 M, find hydroxide ion concentration?

A: Given: [H3O+] = 4.5 x 10-9 M  Hydronium ion is an acid and acid's have low pH which lies in between…

Q: Classify each aqueous solution as acidic, basic, or neutral at 25 °C. Acidic Basic Neutral Answer…

A: At 25°C ;  pH + pOH = 14.0 pH = -log[H+]  pOH = -log[OH-]

Q: Classify the compounds as a strong acid, weak acid, strong base, or weak base. Strong acid Weak acid…

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Q: Calculate the pH of HNO3 solution whose hydrogen ion concentration is 0.76 M. (Round-off your answer…

A: PH= - log [H+]  Where [H+] = concentration of H+ ion

Q: What is the pH of a 1 x 10-5 M NAOH solution? Your Answer:

A: pH is defined as " The negative logarithm to the base 10 of concentration of H+ ions expressed in…

Q: The pH of a 1.1M solution of propanoic acid (HC,H,0,) is measured to be 2.41. Calculate the acid…

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Q: What is the pH of a solution when [-OH] = 10-12 M? Group of answer choices pH = 0 pH = 2 pH = 10 pH…

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Q: Which solution below is the most acidic? Group of answer choices [H3O+] = 1.0 × 10–10 M [H3O+] = 1.0…

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Q: Match the following descriptors to their meaning as it applies to the acidity of a wine.  Soft…

A: Wine is a mixture of ethyl alcohol and water. A wine has a fruity flavor. It has a smooth mouthfeel.…

Q: What is the pH of a 0.039 M HNO3 solution? Your Answer: Answer

A: In this question, we want to determine the the pH of HNO3 Solution.  How we can determine, you can…

Q: Show your work for the question above: "12. What is the pH of a solution in which [OH] = 0.000005…

A: Given in the question , [OH-1] = 0.000005 m pH = 14 + log[OH-1]

Q: Determine the pHpH for the following solutions: [OH−]=5.8×10−4M[OH−]=5.8×10−4M Express your answer…

A: pH is equal to negative logarithm of hydrogen ions

Q: Calculate the pH of a solution containing a caffeine concentration of 415 mg/L. Express your answer…

A: Given : We have to calculate the pH.

Q: A solution was prepared with 3.2 x 10-11 M [H+].  Is this solution acidic or basic? Group of answer…

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Q: Classify each reactant and product in the reaction as an acid or base according to the Brønsted…

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Q: Calculate the pH of a 5.3 M solution of alloxanic acid. Round your answer to 1 decimal place.

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Q: Calculate the pH of a 0.094 M solution of formic acid, H2CO2. The Ka of formic acid 4 x 10-4 Submit…

A: In case of weak acids , the H+ ion concentration is given by the following formula  [H+] = (Ka×C)1/2…

Q: Determine the pka of an acid whose concentration is 0.100M and pH is 2.86.

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Q: What is the concentration of OH ions in a HCl solution whose hydrogen ion concentration is 1.3M?…

A: Given: The concentration of the hydrogen ion in the HCl solution = 1.3 M We have to calculate the…

Q: Fill in the rest: (Use only the exponent for H and OH) pH:  H+:  pOH:  OH-: 10-4

A: [OH-] = 10-4 (given )  pOH = - log [OH-]  pOH = - log (10-4)  pOH = 4  Since, we know that ; pH +…

Q: Choose the correct answer: Which of the following is the strongest acid? HO. HO. HOH CI Br II II Но…

A: COMPOUND SHOWN IN - OPTION -II (FLUORINE DERIVATIVE) IS THE MOST ACIDIC ONE AMONG THE MENTIONED…

Q: Calculate the pOH of the following solutions: (i) 8.24 x 10-3M KOH (ii) 3.98 x 10-2 M Mg(OH)2 A.…

A: Solution (i) pOH = -log[OH-] Since KOH shows 100% dissociation [OH-] = Molarity of KOH = 8.24 x…

Q: i need help solving part a and b of this question please

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Q: Classify each aqueous solution as acidic, basic, or neutral at 25 °C. Acidic Basic Neutral Answer…

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Q: What is the pH of a 0.306 M HNO3 solution? Your Answer:

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

Q: What is the pH of a 0.0515 M NaOH solution? Your Answer:

A: Given [ NaOH]=[OH]=0.0515 we have to find pOH

Q: When the concentration of H3O+ is 6.5 x 10-7 the solution is an acid, a base or neutral.  Choose the…

A: pH of a solution can be calculated by taking the logarithm of the concentration of hydronium ions in…

Q: What is the H+ concentration in M, of a solution that has a pH of (7.5x10^0) ?  (answer to 2 s.f.)

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Q: Find the pOH of a solution whose pH is 11. Answer:

A: pOH of the solution will be 3

Q: Calculate the pH of a 0.50 M tartaric acid solution (pK₁1 = 2.89; pK₂2 = 4.40). Express your answer…

A: Given data :  1. Concentration (c) = 0.50 M  2. pKa1 = 2.89  3. pKa2 = 4.40  To calculate : pH

Q: If the Kb value for a weak base is 2.6*10^-4, what is the value of its conjugate acid?

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Q: QUESTION 11 (4c-401) Which of the following solutions is most basic? Show all work to support your…

A: Basic solutions are those which have pH values of more than 7. Higher is the pH value more it will…

Q: Calculate the pH of a 0.0820 M propionic acid solution.     2.99     2.16     The answer is not…

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Q: What is the pH of a 0.485 M HNO3 solution? Your Answer: Answer

A: Ans. PH = 0.314

Q: [OH-] = 7.9 x 10-3 M Express your answer using two dècimal places. ΑΣΦΦ pH =

A: Given that:  [OH-] = 7.9 × 10-3 M

Q: You may want to reference (Pages 399 - 405) Section 11.6 while completing this problem. Part A A…

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Q: Would you expect a solution containing 0.10M HA2- to be acidic, basic, or neutral?  Explain your…

A: The question is based on the concept of chemical equilibrium. We have to identify the nature of the…

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.