A certain weak base has a Kb of 8.60×10−7M. What concentration of this base will produce a pH of 10.37?

Q: What is the pH of a solution with a hydroxide ion concentration of 10-2 M?

A: [OH-] = 10-2 M  pOH = - log [OH-] pOH = - log (10-2) = 2 At room temperature; pH + pOH = 14 pH + 2 =…

Q: Consider some common drinks. Organize this list of foods with pH from most basic to most acidic.…

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: Calculate the pH of a solution that has [ OH-] = 5.2 x 10-7 M pH=  _?_

A: Given, Concentration of OH-, [OH-] = 5.2*10-7M. The pOH of the solution can be calculated as…

Q: Determine the pH of the following: a single solution prepared to final concentrations of 0.01469 M…

A: pH is the negative logarithm of hydrogen ion concentration. When an acid is mixed with a base, both…

Q: Calculate the pH that results when the following solutions are mixed: 35 mL of 0.20 formic acid, 55…

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Q: Consider a solution that contains both NH3 and NH4NO3. If a solution has a pH of 7.70, calculate the…

A: When a solution contains weak base and its salt with strong acid, a buffer is formed. Such a…

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

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Q: Determine the pH of the following solutions: 1.    [H+1] = 2.3 X 10-13 M 2.    [H+1] = 7.3 X 10-3…

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Q: Which of these solutions has the lowest pH? Rank these solutions: 0.10 M HIO, 0.10 M H2SO4, 0.10 M…

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Q: (a) When 6.3 g of nitric acid are dissolved in water to produce 500.0 mL of solution, what is the…

A: pH of solution is defined as the concentration of hydronium ion H3O+ present in the solution.

Q: Which one of the following 1.0 M solutions would have the lowest pH?

A: D option is right. HF Ka provides a way to gauge the strength of an acid. Larger values signify…

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

A: Given Hydrogen ion concentration is [H+]=4.5×10-10M As we know, pH=-log[H+] pH=-log[4.5×10-10]use…

Q: The pH of a solution is 2.45. What is the molar concentration of hydronium ions in the solution?…

A: We have given that  pH = 2.45  [H3O+] = ?

Q: Find the pH of a KOH solution made by mixing 123 mg KOH with enough water to make 250 cm3 of…

A: Formula used:- pOH = 14-pH

Q: The pH of 30 cm³ of an acidic solution is 2.89. Calculate the concentration of hydrogen ions and the…

A: pH = 2.89  Volume of solution = 30 cm3  We need to find concentration and number of moles of…

Q: A solution in which [H+] = 10-3 M is whereas a solution in which [H+] = 10-10 M is +. Give the pH…

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Q: What is the pH of a solution that has [OH–] = 6.92x10-11 M.

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Q: Determine the pH of each solution. a. 0.0650 M HNO3 c. 0.0195 M KOH b. 0.150 M HNO2 d. 0.245 M…

A: Hi, since you have posted questions with multiple subparts. We will answer the first three subparts…

Q: A certain weak base has a K, of 7.50 x 10-. What concentration of this base will produce a pH of…

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Q: What is the pH of a 0.00100M

A: Negative logarithm of H+ is called pH, to know the acidity of dilute solutions pH is introduced. pH…

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

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Q: Please help me, double check your answers as previous tutors got it wrong.

A: pH is the potential of the hydrogen or the power of the hydrogen. It basically explains how acidic…

Q: Calculate the pH of each of the following aqueous solutions: a. 2.17 x 103 M HCI b. 0.150 M HNO,…

A: Ca (CN)2 is the salt of a weak acid HCN and strong base, Ca (OH)2. Similarly, sodium acetate is a…

Q: Determine the pH of each solution.a. 0.0650 M HNO3 b. 0.150 M HNO2 c. 0.0195 M KOH d. 0.245 M…

A: Given:-              To determine the pH of solution  a. 0.0650 M HNO3 b. 0.150 M HNO2 c. 0.0195 M…

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.90. What is the Kb of this…

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Q: Determine the pH of each of the following solutions: (a) 0.723 M CaCl2 (b) 1.55 M C6H5N (c) 0.00443…

A: Since you have posted a question with multiple subparts, we are entitled to answer first three…

Q: A certain weak base has a Kb of 8.40×10−7. What concentration of this base will produce a pH of…

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Q: Calculate the pH of the solution.  Assume 1.0 L of solution. You must identify the type of solution…

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Q: an aqueous solution has an OH- concentration of 5.753 x 10^-3 M. calculate the pH of this solution.

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Q: classify the solution as acidic, basic, or neutral. [H3O*] [OH] pH РОН Classification 6.3x 104 2.5x…

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Q: Which one of the following 1.0 M solutions would have the lowest pH?

A: Ph= -log [H+] [H+]= 10-14÷[OH-] Lowest PH=C5H5N  (1) For C5H5NOH- = k6xC = 1.7 x 10-9x1…

Q: cle the solution that is most acidic in the list below. Aqueous HCI, pH 1.0 NaOH(aq), pH 11.5 Water,…

A: Solution : pH       pH is a quantitative measure for the acidity or basicity of the solution. This…

Q: 2. Complete the following table: [H;O*] [OH] pH Solution is acidic, basic or neutral 4.56 X 102 3.5…

A: In the given problem we are required to complete the table in which we have to calculate the pH,…

Q: .94g of sodium hydroxide is dissolved in enough water to make 620.0mL of solution at 25 degree…

A: Molecular weight of sodium hydroxide (NaOH) = 23+1+16 = 40 gm/mol  If 40 gm NaOH is present in 1000…

Q: Calculate pH of the following solutions: 0.25 M HNO3 in 0.065 M CH COOH (K.=1.75x10).

A: Solution: We know the common ion aslo affect on oH of the solution. Here first we need to draw an…

Q: What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179…

A: Given : Percent by mass of HCl = 36.0 % Density of solution = 1.179 g/mL Volume of HCl solution to…

Q: Which diagram best represents an aqueous solution of NaF? Will the solution be acidic, basic, or…

A: NaF is a salt , so first we would write its raction with water to check the species formed .  Based…

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: Determine the pH of each of the following solutions. 0.115 MM HCIO2 4.5×10¬2 MM Sr(OH)2 8.58x10-2 MM…

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Q: A certain base has a Kb of 7.8 × 10-6 . What concentration of the base will produce a pH of 11.32?

A: Fristly we calculate the concentration of OH- from the pH : pOH = 14-pH  = 14-11.32 =2.68…

Q: A certain weak base has a Kb of 7.20×10-7. What concentration of this base will produce a pH of…

A: Since it is not given whether the base is monoprotic or not. Hence I'm assuming it to be monoprotic…

Q: Calculate the pH of each solution. H3O+][H3O+] = 6.0×10−7 M

A: pH  calculation using concentration of H+ :

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: You have a 7.4x10-4M Sr(OH)2 solution. What is the pH of this solution?

A: First of all we will calculate pOH then pH

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

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Q: determine the pH of a 0.0006 M NaOH solution

A: We know that, Negative logarithm of H+ ion is know as pH. pH= -log[H+] & pH + pOH =14 & pOH…

Q: 500.0 mL of HCl gas at 27∘∘C and 750.0 mmHg completely dissolves in 100.0 mL of pure water, what is…

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Q: Define and give an example of (a) A weak acid, (b) A weak base

A: Definition of weak acid and weak base with example is given below

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.