Calculate the pH of .50M NH3 when .20M NH4Cl is added

Q: A solution contains 0.377 M potassium acetate and 8.75×10² M acetic acid. The pH of this solution is

A: Given :-  concentration of potassium acetate = 0.377 M  concentration of acetic acid = 8.75 × 10-2 M…

Q: The ?a of a weak monoprotic acid is 1.48×10−5. What is the pH of a 0.0922 M solution of this acid?…

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Q: A solution contains 0.459 M sodium cyanide and 0.269 M hydrocyanic acid. The pH of this solution is

A: Given [NaCN]=0.459M [HCN]=0.269 PH =PKa+log( [NaCN] / [HCN] ) Ka= 6.2*10-10   ( from data ) PKa=…

Q: Listeh A 250.00 mL sample of sulfuric-acid has a pH of 3.54. What is the value of for this solution?…

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Q: A solution contains 0.408 M sodium acetate and 0.145 M acetic acid. The pH of this solution is

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Q: 80.0 mL of 0.30 M NaOH and 80.0 mL of 0.30 M HCl are mixed together. What is the approximate pH of…

A: Acid and base react with each other and form salt and water it is a neutralization reaction In this…

Q: Given, pH of a solution Á is 3 and is mixed with another solution Bhaving pH 2. If both are mixed,…

A: Introduction: The given data : The pH of the solution A = 3 The pH of the solution B = 2 To…

Q: 30 ml of a 0.4375 M HCl solution are added to 35 ml of 0.250 NaOH solution. What is the final pH ?

A: given :-  molarity of HCl solution = 0.4375 M  volume of HCl solution = 30 mL  molarity of NaOH…

Q: A solution containing 572.0mL of 0.6300MHCl is diluted to a volume of 1.000L. What is the pH of this…

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Q: A chemist dissolves 682. mg of pure potassium hydroxide in enough water to make up 70. mL of…

A: A chemist dissolves 682 mg of pure potassium hydroxide in enough water to make up 70mL of solution.…

Q: 3.3. Calculate the pH of the solution prepared by adding 35.00 mL of 0.4211 M NAOH and 63.00 mL of…

A: (3.3)  Given -  Molarity of strong base, sodium hydroxide, NaOH = 0.4211 M  Volume of NaOH = 35.00…

Q: Is it possible that a weak acid solution and strong acid solution have the same pH? Explain.

A: Weak acid-  Acids which do not dissociate completely in aqueous solution. Example - HCl Strong…

Q: A solution contains 0.131 M sodium cyanide and 0.359 Mhydrocyanic acid. The pH of this solution is

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Q: 25.0 g sample of CH3COONa is completely dissolved in 500.0 mL of water and CH3COOH has an acid…

A: Given: Mass of CH3COONa = 25.0 g. And volume of solution = 500.0 mL = 0.500 L…

Q: PRE A Enough of a monoprotic acid is dissolved in water to produce a 1.55 M solution. The pH of the…

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Q: Calculate the theoretical pH for the following solution: . 0.20 M HCl

A: PH= - log [H+]  PH  scale  introduced by Sorensen  Negative logarithm of H + ion concentration known…

Q: Calculate the molarity of the resulting solution if  0.629 grams of Hydrogen ion [H+] is dissolved…

A: Molar mass of Hydrogen = 1.008 gm Mass = 0.629 gm

Q: The pH of an aqueous solution at 25°C was found to be 5.80. The pOH of this solution is .????? The…

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Q: A solution is prepared by mixing 25 mL of 0.06 M NaOH with 65 mL of 0.125 KOH. What is the pH of…

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Q: Determine the pH of a solution that is 0.20 M in NH3 and 0.30 M NH4Cl

A: The mixture of NH3 with NH4Cl is a buffer solution as it is a mixture of weak base (NH3) with its…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0184 M solution. The pH of the…

A: Acids are the compounds which donate protons, H+ in the solution. Weak acids partially dissociate…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.16 M solution. The pH of the…

A: Given, the concentration of the monoprotic acid = 1.16 M pH of the solution of monoprotic acid =…

Q: Calculate the following:  1) [OH-] and molarity M of an HCL solution with pH= 3.4  2) Resulting…

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Q: In the laboratory, a general chemistry student measured the pH of a 0.591 M aqueous solution of…

A: Dear student I have given answer to your question in the image format.

Q: 0.0155L of a 0.505M solution of HCl is combined with 0.0482L of a 0.0175M solution of NaOH. What is…

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Q: The pH of a solution that contains 1.2M acetic acid and 0.920M sodium acetate is?

A: pH of weak acid = 4.63.

Q: A solution contains 0.355 M ammonium chloride and 7.65×10² M ammonia. The pH of this solution is

A: Mixture of Ammonium Chloride and Ammonia is a basic buffer solution. It's pH can be calculated by…

Q: A 0.020 M solution of niacin has a pH of 3.26. Calculate the percent ionization of the niacin.

A: Given information: pH = 3.26 Concentration of acid = 0.020 M

Q: The ?a of a weak monoprotic acid is 1.45×10−5. What is the pH of a 0.0784 M solution of this acid?

A: The weak acid dissociation is written as:

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.76 M solution. The pH of the…

A: Given :-  Concentration of monoprotic acid = 1.76 M  pH of solution = 2.61  To be calculated :-  Ka…

Q: Calculate the pH of the following solution: 1.0 M HI

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Q: A solution is made by mixing 0.05 mL of 1.0 M HCI with 999.95 mL of pure water. Calculate the pH of…

A: The pH of a solution is the negative logarithm of hydrogen ion concentration.

Q: Calculate the pH when 29.91 mL of 0.2628 M carbonic acid is mixed with 10.1 mL of 0.1448 M NaOH.

A: For carbonic acid, 29.91 mL of 0.2628 M carbonic acid Ncarbonic acid  = n- factor × M…

Q: the pH when15 mL of 0.25 M HClO4 are added to 25 mL of 0.20 M NaOH.

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Q: A solution contains 0.129 M ammonium chloride and 7.45x102 M ammonia. The pH of this solution is

A: Given :-  [NH4Cl] = 0.129 M  [NH3] = 7.45 × 10-2 M  To calculate :  pH of solution

Q: An aqueous solution contains 0.372 M KHS and 0.361 M H,S. The pH of this solution is

A: As per our guidelines, we are supposed to answer?️ only one question. Kindly repost other questions…

Q: A solution is prepared by mixing 0.2 moles of HCl into water until the final volume of the solution…

A: pH = -log[H3O+]  This formula is used to calculate to pH .

Q: For a weak acid in solution (HA), how would adding a substance containing a common ion (A) affect…

A: When the solubility of a sparingly soluble compound decreases in presence of another compound having…

Q: A solution contains 0.342 M sodium acetate and 0.112 M acetic acid. The pH of this solution is .

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Q: 2. 30 mL of a 0.4375 M HCI solution are added to 35 mL of 0.250 NAOH solution. What is the final pH?

A: Given: The volume of HCl = 30 mL The concentration of HCl = 0.4375 M The volume of NaOH = 35 mL The…

Q: 4. 4.00 g KOH was added to the less basic solution in number 3. What will be the resulting pH of the…

A: Given, Mass of NaOH = 5.00 g  Mass of Ba(OH)2 = 5.00 g  Gram molar mass of NaOH = 40 g/mol  Gram…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.74 M solution. The pH of the…

A: Let, HA be the monoprotic acid. Given, concentration of monoprotic acid, [HA] = 1.74 M     and, pH =…

Q: If 1.0 mL of 0.4 M HCl was added to 40.0 mL of pure water, what would the resulting ΔpH of the…

A: Since moles of HCl taken = volume of HCl in L X molarity of HCl = 0.4 X 1 / 1000 = 0.0004 Since HCl…

Q: A solution contains 0.251 M potassium cyanide and 0.454 M hydrocyanic acid. The pH of this solution…

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Q: Enough of a monoprotic acid is dissolved in water to produce a 1.67 M solution. The pH of the…

A: 1- First calculate the H+ ion Concentration :  We know that, pH = -log([H+])  -pH = log([H+])  [H+]…

Q: Which of the following is the weakest acid? HOI    HOCl    HOBr    Since they are all oxyacids,…

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Q: You have a 0.125 M solution of ammonium chloride.  If the Kb of NH3 = 1.75x10-5, calculate the pH of…

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Q: The pH is dependent on which of the following? acid concentration Owhether the acid is strong or…

A: To find: if pH of  solution is dependent on the acid concentration or the strength of the acid.

Q: What is the pH of a 0.20M solution of HCN and the % of ionization if my Ka is 4.9x10^-10?

A: Given: The concentration of HCN, (C) = 0.20 M  The dissociation constant of HCN, (Ka) = 4.9×10-10…

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.