Calculate the Ka and Kb values for 1.0 M NaHSO4 and Na2CO3

Q: Calculate the pH value of a solution consisting of 100 mL of KOH 10^-1 mol/L and 100 mL of CH3COOH…

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Q: How many moles of HA would need to be added to 481 mL of 0.816 M NaA to produce a solution with a pH…

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Q: A 0.045 0 M solution of HA has a pH of 2.78. Find pKa for HA.

A: Given, initial concentration of HA = 0.0450 M             pH = 2.78 We know that, pH can be…

Q: 4. Citric acid has three Ka values, Kal = 7.4 x 10-4, Ka2 = 1.7 x 10-5, and Ka3 = 4.0 x 10-7. Write…

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Q: Calculate the pH at 25 °C of a 0.80 M solution of potassium butanoate (KC, H,CO,). Note that…

A: Given,  [KC3H7CO2] = C = 0.80 M  pKa value of HC3H7CO2 = 4.82  Calculate the pH = ?

Q: How many grams of acid are needed to prepare a 0.1 M 100 mL phosphate buffer solution with a pH of…

A: We need to prepare phosphate buffer solution with a pH of 7.4

Q: How many moles of NaA would need to be added to 512 mL of 1.28 M HA to produce a solution with a pH…

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Q: The pH of 0.17 M of HCN is Ka of HCN = 1.6 x 10 10 %3D (Write your answer to 2 d.p. eg: 7.65)

A: The question is based on the concept of chemical equilibrium. we have been given a weak acid…

Q: Calculate the percent ionization for bromic acid in a solution that contains 0.00850 M acetic acid…

A: Concentration of acetic acid, HC2H3O2(aq) = 0.00850 M For acetic acid, HC2H3O2(aq), Ka = 1.8×10–5,…

Q: 0.30 M solution of a salt NaA has pH=9.01pH=9.01. What is the value of Ka for the parent acid HA?

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Q: Specify the formal charge at each of the labeled atoms, a - c, in each of the following structures.…

A: Formal charge = Total number of valence electrons- total number of lone pair electrons -(total…

Q: 10 10 mL 0.05 M NAOH Hd

A: Henderson's equation: pH = pKa + log[salt]/[acid] at equivalent point: [salt] = [acid] pH = pKa

Q: What is the pH of a solution that is 0.12 M in HOCl and 0.20 M in NaOCl?  Ka of HOCl is 3.5 x 10-8…

A: Given, 0.12 M in HOCl and 0.20 M in NaOCl

Q: You have an aliquot of 10 mL of 0.1022 mol/L phosphoric acid.  The ka values for phosphoric acid are…

A: The objective of this question is to calculate the resultant pH of a solution after mixing…

Q: A 0.100 M solution of the salt BHX has a pH of 8.00, where B is a weak base and X- is the anion of…

A: As per the given information BHX is dissociate in solution to produce BH+and X- ions. because the…

Q: 9) HB has a Ka of 5.2 x 10-5 and HC has a Ka of 4.6 x 10-4 . Which solution will have a lower pH,…

A: Given : Ka of HB = 5.2 X 10-5  Ka of HC = 4.6 X 10-4  And concentration of HB = concentration of HC…

Q: You have an aliquot of 12 mL of 0.1010 mol/L phosphoric acid.  The ka values for phosphoric acid are…

A: The objective of this question is to calculate the resultant pH of a solution after mixing…

Q: A 0.3654 g portion of pure formic acid (CH2O2, FW=46.03 g/mol, Ka=1.77 x 10-4) is dissolved in 50.00…

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Q: You have an aliquot of 11 mL of 0.1093 mol/L phosphoric acid. The ka values for phosphoric acid are…

A: Volume of phosphoric acid = 11 mLMolarity of phosphoric acid sample = 0.1093 mol/LVolume of NaOH…

Q: A solution of 0.05 M in NH4CI and 0.03M in NH3, calculate its OH- concentration and its pH. (pKa…

A: Concentration of NH4+ = [NH4+] = 0.05 M Concentration of NH3 = [NH3] = 0.03 M OH- concentration of…

Q: Calculate the pH of a solution containing 0.3 M HCOOH and 0.1 M HCOO (pKa of HCOOH = 3.76)

A: Concentration of HCOOH (Acid) = 0.3 M  Concentration of HCOO- (conjugate base of acid) =  0.1 M  pKa…

Q: What mass of NaA (MW=100 g/mole) must be added to a 100.0 ml of a 0.1 M solution of HA (Ka=1x10-5)…

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Q: Phosphoric acid is a triprotic acid with the Ka values of 7.25 10-3, 6.31 10-8 and 3.98 10-13…

A: Millimoles of H3PO4 taken   =Molar concentration of acid×Volume of acid=0.1000 M×25 mL=2.5 mmol

Q: You have an aliquot of 10 mL of 0.1094 mol/L phosphoric acid.  The ka values for phosphoric acid are…

A: The objective of this question is to calculate the resultant pH of a solution after mixing…

Q: How many grams of NaA (57.93 g/mol) would need to be added to 590 mL of 1.17 M HA to produce a…

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Q: What is the pH of a solution that is 0.0032 M in HA and also 0.087 M in NaA? (Ka = 4.1 × 10-6) 6.56…

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Q: If the ph of  24.0 ml of 1.0 M NaOAc is added to 1.0 M of HOAc is 4.97, what's the equilibrium [H+]…

A: The value of pH is given by the following equation pH= -log [H+] Or,  [H+] = 10-pH pH of a buffer…

Q: . If BaCl2 completely dissolves in water, what is the ionic strength of a 0.0300 F solution of…

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Q: which of the following expressions is the correct equilibrium constant expression

A: We have to select the correct expression for equilibrium constant for the given expression

Q: What is the pH of a 0.375 L solution made with and 25.00 mL of 5.50 M HBRO (K, = 2.3 x 10 ) 2.775 g…

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Q: calculate the pH of the equivalence pount concentraton of N2OH solution = oil mollL Mean tire (NoOH…

A: Aspirin is a weak acid. It is reacting with a strong base NaOH. So, the equivalence point will be…

Q: Calculate the pH of a buffer solution prepared by dissolving 0.83 mole of acid, HA, and 0.67 mole of…

A: Given data is as follows: The number of moles of HA acid = 0.83 mol The of moles of salt NaA = 0.67…

Q: Calculate the pH of a solution that contains 0.10 m HC2H3O2 and 0.050 m NaC2H3O2. The Ka for HC2H3O2…

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Q: What volume of 0.1543 M NaOH must be added to 25.00 mL of 0.2405 M HCOOH in order to prepare a…

A: Ka = 1.8 ×10–4 pKa = – logKa = – log(1.8 ×10–4) = 3.745 Let n be the number of millimoles of NaOH to…

Q: Item 14: Question Calculate the pH of a solution prepared by dissolving 2.129 g of solid anhydrous…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Calculate the pH of a buffer solution that prepared by dissolving 0.025 mole of CH3COOK and 0.020…

A: To calculate the pH of buffer solution use formula which is given below. pH=pKa+log[Salt][Acid] Here…

Q: You have an aliquot of 11 mL of 0.1045 mol/L phosphoric acid.  The ka values for phosphoric acid are…

A: The objective of this question is to calculate the resultant pH of a solution after mixing…

Q: A salt (MA) is dissolved in water. Given the values of ka and kb below, would the salt be considered…

A: If kb is greater than ka then solution is basic . And if ka is greater than kb then solution is…

Q: 1. Calculate the concentration of sodium benzoate (NaC,H,O) that must be present in a 0.20M solution…

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Q: Calculate the pH of a solution containing 0.03 M NaH2VO4 and 0.05 M Na2HVO4. (Ka1 = 1.11×10-2, Ka2 =…

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Q: What is the pH of the solution that is prepared by dissolving 0.8 g of lactic acid (90.08 g/mol, Ka…

A: We have given that  What is the pH of the solution that is prepared by dissolving 0.8 g of lactic…

Q: A certainvinegar is found to contain 5.7% acetic acid CH3COOH by mass. What mass of this vinegar…

A: The Molarity of original starting Solution, containing 5.7 % Acetic acid by mass ,can be calculated…

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.