-9. Calculate the pH of a 7.5 x 10 M aqueous solution of hydrochloric acid (HC1).

Q: What is the pH of the solution that results from adding 59.8 mL of 0.150 M HCe to 22 mL of 0.650 M…

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Q: What is the pH of a 0.20 M solution of a generic weak acid? The Kb value for this generic weak acid…

A: Given data  kb = 4.0 x 10-5 concentration, c= 0.20 M Formula used       OH- = kb×cpOH =…

Q: Show complete calculations for the pH of a 0.115M solution of ammonia. The Kb for ammonia is 1.8 x…

A:

Q: What is the pH of a 0.122 M monoprotic acid whose K, is 5.7 x 104? a

A: question given concentration and Ka using this we can calculate the degree of dissociation  using…

Q: Enter your answer in the provided box. Determine the K, of a weak base if a 0.29 M solution of the…

A: The pOH of 0.29 M solution is calculated below.

Q: At 25°C, calculate the pH of a 0.426 M solution of the salt KNO2. (Ka (HNO2) = 4.50 × 10−4 ).

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Q: 1    Calculate the pH of a 0.02 M solution of the weak acid, HA.         Ka = 2.46 X 10 –4…

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Q: What is the pH of a solution prepared by dissolving 8.50 g C6H5NH3^+Cl^-in 750 mL of 0.258 M…

A: Given data is as follows: The mass of C6H5NH3+Cl- = 8.50 g The volume of C6H5NH2 = 750 mL The…

Q: Enter your answer in the provided box. Calculate the pH at 25°C of a 0.25 M aqueous solution of…

A: Given data:

Q: NH3 is a weak base (?b=1.8×10^−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Given: Kb = 1.8 × 10-5              Concentration of solution = 0.056 M             Temperature = 25…

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: Calculate the pH of a 100.0 mL solution containing 9.06 g KClO

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: Determine the pH of a 0.100 M aqueous solution of NaOcI. Data: pK,[HOCI] = 7.40 А 10.20 B 9.75 C…

A: 1- First we will see the Ka from its pKa :  pKa = -log(Ka)  -pKa = log(Ka)  10-pKa = Ka  Ka =…

Q: Calculate the OH- for a 0.300 M solution of pyridine, Kb = 1.7 x 10^-9

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Q: Calculate the pH of a 0.100 M solution of a weak base, A-, given Kb = 6.38×10-6.

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Q: Which of the following is the pH of the solution containing 0.01 mol CH3COOH and 0.820 grams of…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: What is the pH of a solution that is 0.15 M NH4Cl and 0.35 M NH3?   The Ka of NH4Cl is 5.01 x…

A: In this question , we have to calculate the correct pH of given problem by the help of…

Q: What is the pH of an aqueous solution that is 0.123 M NH4Cl? (Kb for NH3= 1.8 x 10^-5)

A: Solution :         The pH of an acid or base can be calculated by using hydronium ion…

Q: Acid rain is due to the dissolution of sulfur oxide (SO3) present in contaminated areas in the…

A: The reactions taking place are-

Q: What is the pH of the solution containing 0.01 mol of CH3COOH and 0.820 grams of NaCH3COO in 100 mL…

A: Calculation of pH.

Q: he hypochlorite ion, OCl-, is commonly found in bleaches and other disinfectants used in swimming…

A: Chemical reaction HOCl      →      H+        +       Cl-Initial                          0.1 M…

Q: What is the pH of a 0.144 M solution of ammonia (Kb 1.8 x 10-5)?

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Q: Calculate the pH of a solution with [OH]] of 6.58×106. pH = %3D

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Q: How many moles of NH3 must be dissolved in water to give 813.0 mL of solution with a pH of 11.15? Kb…

A: The value of Kb for the given weak base is = 1.8x10-5 The concentration of the base solution is =?…

Q: Ammonia is a weak base that is a household cleaner and has a Kb =1.8 x 10-5. What is the pH of a 3.0…

A: Given: Kb =1.8 x 10-5Concentration = 3.0 M pH = ?

Q: A solution of acetic acid (Ka = 1.8 × 10‒5) has a pH of 2.65. What is the concentration of acetic…

A: Given information: Ka of acetic acid = 1.8 × 10‒5 pH is 2.65

Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…

A:

Q: Calculate the ph of 0.350 M acetic acid whose ionization constant is Ka= 1.8x10-5

A: Given :-  concentration of acetic acid solution = 0.350 M  Ka = 1.8 × 10-5  To be calculated :-  pH…

Q: The pH of a solution at 25°C in which [OH]=2.0 x 10 is: 4.69 9.30 3.30 4.76 9.52

A: hydroxide ion concentration can be used to find pOH which then be used to find the pH.

Q: Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a…

A:

Q: Find the pH of a solution that is 0.25 M in formic acid, and 0.33 M in sodium formate. K, for formic…

A: Given  Ka = 1.7 × 10-4 Concentration of HCOOH = 0.25 M  Concentrate of HCOONa  = 0.33M PH = ? PKa =…

Q: HCN is a weak acid (Ka = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0675 M we have to determine the pH ? Kb = Kw / Ka       = 1 ×…

Q: 2) Determine the pH of a solution by adding 0.23 mole formic acid and 0.17 mole of sodium formate in…

A: Henderson Hasselbalch equation is given by, pH=-log(Ka)+log[salt][acid] where Ka is the acid…

Q: Calculate the pH of 0.750 M pyridinium chloride, C5H5NHCl? Given Kb of C5H5N is 1.70×10-9.

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Q: 1. Calculate the pH of a 0.045M sulfurous acid solution. H,SO, → H* + HSO, Ка, = 1.7 x 102 HSO3- H +…

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Q: Based on the Kb determined in the previous part, what is the pH of the initial 1.0 M base solution?…

A:

Q: HCNN is a weak acid (?a=6.20×10^−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0525 M we have to determine the pH ? Kb = Kw / Ka       = 1 ×…

Q: Calculate the pH of a solution containing 0.20 M HN3 and 0.30 NH4Cl, Kb=1.8x10-5

A: pOH of a solution containing salt and base can be calculated by using the equation :…

Q: What is the pH of a 3.0 x 10 M solution of CoHsNH2 (Kb= 4.3 x 1010? What is the percent error in…

A: As PhNH2 is an weak base,it can be calculated using a formula.

Q: What is the pH of a 1.0 x 10 M BalOH), solution at 25 °C: 7

A:

Q: Calculate the pH of 3.0 X 10-5 M Mg(OH)-, which completely dissociates to Mg2+ and OH-.

A: Given that the Mg(OH)2 completely dissociates, so the dissociation reaction is, Mg(OH)2 →Mg2++2OH-

Q: A sample of rain water is tested and found to have a pH of 4.52.  What is the pOH of this rain…

A:

Q: NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Dissociation constant of base is given by,

Q: What is the pH of a solution of 0.30 M CH:NH:Cl? Kb for CH:NH2 = 4.4 x 104

A:

Q: what is the pH of a solution prepared by adding 78.69 mL of 0.100 M sodium hydroxide to 50.9 mL of…

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Q: -8. Calculate the pH of a 5.1 x 10 °M aqueous solution of hydroiodic acid (HI).

A: Given :- concentration of HI = 5.1 × 10-8 M  To calculate :- pH of the solution  pH = -log [H+]

Q: What is the pH of a solution that is 0.025M formic acid, HCHO2, and 0.018M sodium formate,…

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Q: Calculate the pH of a 0.400 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4.

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.