35. Calculate the pH of a solution that is 0.15 M in formic acid (HCOOH) and 0.20 M in sodium formate (HCOONa). The K₂ of formic acid is K₂ = 1.8×10-4. (A) 9.21 (B) 3.87 (C) 4.53 (D) 7.00 (E) 1.15

Q: Calculate the pH and the pOH of each of the following solutions at 25°C for which the substances…

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Q: pH

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Q: 6) Classify each of the following acids as strong or weak. For all the acids, write the dissociation…

A: Given  a) HNO3 Nature of Acid  ( Strong or weak  )  = ?  Dissociation equation in water = ?  b)…

Q: Calculate the [H+] for (a) black coffee with a pH of 4.42 (Enter your answer as follows: 1.0E-2 for…

A: (a) pH can be written as - pH = - log [H+] [H+] = Antilog (- pH) [H+] = Antilog ( - 4.42) [H+] =…

Q: Methylamine, CH3NH2, is a weak base that hydrolyzes water according to the equation shown below. The…

A: Given :  Concentration of methylamine = 0.225 M  Kb of methylamine= 5.2 x 10-4

Q: Calculate the pH and the pOH of each of the following solutions at 25°C for which the substances…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Consider 0.10 M NaCN solution. (a) Show an equation of dissociation (ionization) of NaCN in water.…

A: The dissociation of NaCN in water is as follows :NaCNs ⇌                 Na+aq + CN-aq

Q: 7. If a neutral solution of a water , with pH= 7.00, is cooled to 10oC, the pH rises to 7.27. Which…

A: Water can react with itself in a weak acid-base equilibrium to create hydronium ion and hydroxide…

Q: Which acid is the weakest? (A) HCN (K, = 4.9×10-10) (B) HOCI (K, = 3.5×10-*) (C) HNO; (K, = 4.5×104)…

A: Given :-  A) HCN (Ka= 4.9 x 10-10) B) HOCl (Ka = 3.5 x 10-8)  C) HNO2 (Ka = 4.5 x 10-4) D) CH3COOH…

Q: Phenol, C6H5OH, has a Ka = 1.3x 10 -10 (a) Write out the Ka reaction for phenol (b) Calculate  Kb…

A: Answer:Any specie that loses H+ ion upon adding in water is called Bronsted-Lowry acid and the…

Q: Calculate the pH of the following solutions. (1)Tap water after boiling       (2)  0.0010 M NaOH…

A: Note - Since you have asked a question with multiple sub-parts, we will do the first three sub-parts…

Q: Calculate the pH change that results when 15 mL of 2.0 M HCl is added to 560. mL of each of the…

A: The formula to calculate the pH is

Q: Calculate the [H+] for: (a) black coffee with a pH of 4.88 (Enter your answer as follows: 1.0E-2…

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Q: . (a) Calculate the pH of a 0.20 M solution of benzoic acid at 25°C. (b) How many moles of acetic…

A: pH of a solution tells about the acidity of the solution. It is given by the negative logarithm of…

Q: (a) Calculate the percent ionization of 0.00190 M hypochlorous acid (K₂ = 3e-08). % ionization = %…

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Q: 3. The pH of a 0.10 M solution of hydrazine, H₂NNH2, is 10.54. (a) Is hydrazine a weak base or acid?…

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Q: Determine the pH of the following solutions:   (a) 50.0 mg of naproxen (pKa = 4.2) sodium…

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Q: Calculate the pH of a solution that is 0.15 M in formic acid (HCOOH) and 0.20 M in sodium formate…

A: Given, Concentration of formic acid = [HCOOH] = 0.15 M Concentration of sodium formate = [HCOONa] =…

Q: Chemists use a number denoted by pH to describe quantitatively the acidity or basicity of solutions.…

A: According to the formula :     pH = -logH+  where H+ is the hydrogen ion concentration in moles per…

Q: 13. A 60.00 mL sample of 0.075 M sodium benzoate (NaC7H5O2) was titrated with 0.050 M HCl. What is…

A: Sodium benzoate is a salt and HCl is an acid.

Q: . Which of the following could be added to 50.0 mL of 0.10 mol L¯ª nitric acid solution to change…

A: pH is the measure of hydrogen ion concentration in a solution. It is given as follows; pH = - log…

Q: Calculate the acetate ion concentration in a solution prepared by dissolving 8.70×10-3 mol of HCl(g)…

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Q: 9. What is the pH of a solution whose hydronium ion concentration is 2.5 X 10-8 M? (a) 7.6 (b) 8.0…

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Q: Calculate the pH of a solution when the following quantities of 0.7500 M KOH are added to 60.00 ml…

A: Hello. Since the question consists of multiple sub-parts, the first three sub-parts will be solved.…

Q: Calculate the pH change that results when 14 mL of 2.4 M HCl is added to 510. mL of each of the…

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Q: 4.Indicate whether the following solutions are acidic (A), basic (B), or neutral (N). (a)pH 8.6…

A: (a) pH = 8.6   The nature of solution can be determined from the pH scale as:   pH scale ranges from…

Q: (a)  Calculate the pH of a 0.20 M solution of benzoic acid at 25°C.(b)  How many moles of acetic…

A: pH of a solution tells about the acidity of the solution. It is given by the negative logarithm of…

Q: 7 (a) Describe what happens when each of the following molecules is separately dissolved in water…

A: A conjugate acid–base pair consists of two substances that differ only by the presence of a proton…

Q: In the reaction NH3(aq) + H₂O(1)⇒ NH4*(aq)+ OH¯(aq) does water act as a Brønsted-Lowry acid, a…

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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.