If the K, of a weak base is 7.2 x 10-6, what is the pH of a 0.33 M solution of this base? pH = 4.675 Incorrect

Q: A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H+] = 7.2 x 10-5 M?…

A: Given, the concentration of hydrogen ion for an aqueous solution asfollows, [H+ ] =7.2×10-5we are…

Q: In Experiment 5, Qualitative Test for Anions, the white solid was dissolved when CH3COOH (aq) was…

A: Analysis of anions or cations means that what type of cations or anions are present in a given…

Q: Q4// Calculate the molar concentration for acetic acid that ionized at 2.5%, ka=1 ×10-5 *

A: Degree of dissociation (α) Weak electrolytes ionized partially in aqueous solution. Degree of…

Q: QUESTION 7 At 25°C, the pH of a vinegar solution is 2.60. What are the values of [H 30 and [OH J in…

A:

Q: If the Kp of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH 0.00511…

A: Given : Initial concentration of weak base B = 0.47 M Kb of base = 2.4 X 10-6  Since B is a weak…

Q: A weak base is dissolved in water with a concentration of 0.150 mol/L. The Kb value of the base is…

A: To calculate the pH of a weak base , we would first write its reaction with water . Base would gain…

Q: An acid (HA) dissociates as follows: HA - H* + A minus Arrow should be interpreted as an equilibrium…

A:

Q: B: What is the pH of 0.6 M NH,Cl solution? Discuss your results. (K of NH= 1.8 x 10 NH4+ + H2O+→…

A: Firstly, write the equilibrium constant for the given reaction. It is calculated by dividing the…

Q: 5. If the pH of the methyl red solution is changed to 4, answer with T (increase), v (decrease), +…

A: Given information:

Q: Answer #1 only.

A:

Q: Question 69 What is the pH of the solution if the hydrogen ion (H*) concentration is 1.0 M? 1 10

A: We have to calculate the pH of Solution.

Q: Calculate the pH and the pOH of an aqueous solution that is 0.030 M in HCl(aq) and 0.075 M in…

A: Given-> Concentration of HCl = 0.030 M Concentration of HBr = 0.075 M

Q: Determine the [H+] in a 0.155 M HClO solution. The Ka of HClO is 2.9 × 10-8.

A: Given, Concentration of the H+ ion = [H+] = ? Ka of HClO = 2.9 × 10-8 Concentration of the HClO…

Q: 3. Hydrofluoric acid, HF, has a Ka of 6.8 × 10-4. Determine the pH and POH for a 0.35 M F solution.…

A: Given: Ka of HF is 6.8*10-4 Concentration of fluoride ion = 0.35 M

Q: The pH of an aqueous solution at 25°C was found to be 3.90. The pOH of this solution is The…

A: pH is defined as the negative logarithm of hydrogen or hydronium ion concentration present in the…

Q: What is the pH of a 4.0×10 M solution of KOH at 25 °C? Submit Show Approach Show Tutor Steps

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Q: Q4// Calculate the molar concentration for acctic acid that ionized at 2.5%, ka=1 x10-5

A:

Q: Question 6. Three solutions have the following pH: • Solution 1: pH 7.4, Solution 2: pH 10.6,…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: A 0.200 M solution of an acid, HBrun, has a pH = 1.00. What is the value of the ionization constant,…

A: Let 'x' be the change in the concentration of HBrun. The equilibrium concentrations can be…

Q: 3. State the pH value of a sample that has ten times fewer hydronium ions than an equal volume of a…

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Q: What is the pH of a 0.431 M weak base solution? The K, of the weak base is 0.000026. Your Answer:…

A: Data given: The concentration of the weak base = 0.431 M The equilibrium constant, Kb for the weak…

Q: Question 5 If your pH = 4.2, find [H*) %3D O 1.0 x 10 M O 3.2 x 10 -5 M O 1.0 M 062x 10 M

A: Given, pH=4.2

Q: the pH of a 1.4x 10–6 M Ca(OH)2-solution? 5

A:

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: QUESTION 10 An aqueous solution has a [OH-] = 2.52 x 10-9 M.        a.  What is the pH of the…

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Q: Use: pH = -Log [H30*] 1. Round answers to the tenths place: (show work) a) Find the pH of a solution…

A: pH: It is defined by saying that power of hydronium ions, on the basis of this w can categorize the…

Q: QUESTION 19 Determine the pH of a 0.500 M NH3 solution at 25°C. The K, of NH3 is 1.76 x 103 O 10.281…

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Q: Question 2 What is the pH of a solution when [OH]= 3.8 x 10P. Is this solution acidic or basic? Show…

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

Q: Two students were investigating acidic and basic solutions. Test Bob Sandy Red Litmus Red Red Blue…

A: Litmus are the acid base indicators and we can easily determine if a solution is acidic or basic by…

Q: 4.) Explain what happens to the H* and OH concentrations of a solution when the pH goes from 7 to 4…

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Q: Question 12 What is the pH of a solution prepared by adding 11.0 mL of 1.17 M hydrochloric acid to…

A: hi

Q: calculate strength differences for acids and bases. compare the two solution in each pair, indicate…

A: We know, the acidity or basicity of a compound is determined by the pH value.

Q: In Experiment 5, Qualitative Test for Anions, the white solid was dissolved when CH3COOH (aq) was…

A: Here we have to the cause of dissolution of Barium phosphate in acetic acid but not barium sulfate.

Q: Question 4 A weak base, B, with a a) Calculate the pH of the weak base, B. concentration of 0.150 M…

A:

Q: In Experiment 5, Qualitative Test for Anions, the white solid was dissolved when CH3COOH (aq) was…

A: The quantitative analysis of anion can be understood as-

Q: Question 13 What is the pH of a 0.097 M weak base solution? The K, of the weak base is 0.000017.…

A:

Q: Calculate the hydroxide ion concentration, [OH ], for a solution with a pH of 3.72. 10 x1010 =[_HO]…

A: The given data contains, pH = 3.72

Q: What is the pH of a 0.5M HF solution (at 25ºc)? Ka is 7.1 x 10-4 (Round-off your answer to two…

A: Acids bases and salts topic

Q: What is the pH created when 2.600 L of an aqueous weak monoprotic acid whose molarity is 0.1750 M…

A:

Q: Find pH for [H30+] of 7.9*10^-11 M?

A:

Q: What is the concentration of hydroxide ion in a 0.170 M aqueous solution of hydroxylamine, NH2OH?…

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

Q: Question 22 What is the pH of a 1.537 M acetic acid (CH3COOH) solution? Kg 1.8 10-5 Report your…

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Q: Hint < Question 10 of 21 If the K, of a monoprotic weak acid is 6.3 x 10-6, what is the pH of a 0.27…

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Q: Calculate is the pH of 0.02 M HC2H302? Ka-1.8x10^-5 Your answer

A: 0.02 M HC2H3O2 has a Ka of 1.8 × 10-5 .Here we have to calculate the pH of the solution.

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

A: Ans. PH = 0.314

Q: A solution has a [OH1-] = 4.40 x 10-11 M. Use the self ionization constant of water (Kw) to find the…

A: Water decomposes and gives hydroxide ion and hydronium ion and the equilibrium constant for this…

Q: QUESTION 6 What is the hydronium (H3O*) concentration of a solution with a pH of 5.16?

A:

Q: What is the pH of an aqueous solution that has a hydronium ion concentration of [H3O+]= 1.0 x 10-4…

A: The pH of the solution can be calculated as follows: pH=-logH3O+ H3O+=1.0×10-4 moles/liter

Q: If a solution has a hydroxide ion concentration of 1x10-10, the pH of the solution is? Show work.

A: Given, [OH-] = 1 x 10-10 We know, PH = -log [H+] POH = -[logOH-] POH = - log [1 x10-1] POH = - (log…

Q: Question 4 Find the pH of 1.0 x 10-3 M nitric acid. pH = 4.0 O pH = 2.0 pH = 3.0 O pH = 3.5

A: The answer is as follows:

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.