A weak acid (HCN) solution is mixed with the sodium salt of its conjugate base (NaCN). If the pH of 0.25 M HCN in 0.12 M NaCN is 5.50, calculate the value of K, for HCN.

Q: Explain why the pH does not change significantly when a small amount of an acid or a base is added…

A: Option D is correct

Q: Calculate the pH of(a) a solution that is 0.250 M in sodium formate (HCOONa)and 0.100 M in formic…

A: (a). Given information; The initial concentration of formic acid (HCOOH) is 0.100 M The initial…

Q: A student is given a 0.1 M solution of an acid and is asked to determine whether it is a solution of…

A: Given: Concentration of acid = 0.1 M And the pH of the solution = 2.3

Q: A 0.110 M solution of a weak acid has a pH of 2.84. What is the value of K, for the acid?

A:

Q: 20.0 ml of 0.01 M HCl is added to    5. 6    ml  0. 10 M NaOH, the resulting pH of the solution will…

A:

Q: A weak acid (HCN) solution is mixed with the sodium salt of its conjugate base (NaCN). If the pH of…

A: We have 0.12 M NaCN , 0.25 M HCN and pH as 5.5 , we have to calculate the Ka for HCN.

Q: Explain why the pH does not change significantly when a small amount of an acid or a base is added…

A: The solution of a weak acid or base with its conjugate base or acid respectively is known as a…

Q: The indicator thymol blue changes from red to yellow between pH 1.2 and pH 2.8. If thymol blue is…

A: The objective of the question is to determine the pH and nature (acidic, basic, or neutral) of a…

Q: A solution is prepared that is initially 0.22M in methylamine (CH, NH,), a weak base, and 0.31 M in…

A:

Q: A student is trying to prepare a buffer solution with a pH of 9.00. Calculate the mass of potassium…

A: pH of a buffer is calculated using Henderson -Hasselbalch equation    pH = 9  pka = -log Ka  We…

Q: A solution contains 5.59×10-2 M potassium fluoride and 0.136 M hydrofluoric acid. The pH of this…

A:

Q: A chemist adds a chemical to pure water and there is a 100-fold incre approximation of the new pH…

A: The objective of the question is to calculate the new .

Q: A solution contains 0.420 M CH3NH3 and 0.143 M methylamine, CH3NH2. The pH of this solution is .

A: Given : Concentration of CH3NH3+ = 0.420 M And concentration of CH3NH2 = 0.143 M Since the solution…

Q: A student is provided with a 1.0 M stock solution of hydrochloric acid (HCl) and asked to mix 5.00…

A: The dilution solution is prepared by reducing the concentration of solute in stock solution by…

Q: A weak acid, HCN, is in solution with dissolved sodium cyanide, NaCN.  If HCl is added which ion…

A: A buffer solution is the one whose pH remains unchanged over a range of addition of strong acid or a…

Q: A chemist dissolves 215. mg of pure sodium hydroxide in enough water to make up 170 mL of solution.…

A: Hydronium ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The titration of 50.00 mL of 0.150-M HCl with 0.150-M NaOH (the titrant) is carried out in a…

A: The balanced equation for the reaction between HCl and NaOH is   HCl + NaOH --------> NaCl + H2O…

Q: An analytical chemist is titrating 88.9 mL of a 0.2700M solution of ammonia (NH3) with a 0.4900M…

A: Ammonia, NH3(aq) is a monoacidic weak base with pKb = 4.74 HIO3(aq) is a monoprotic strong acid.…

Q: The indicator thymol blue changes from red to yellow between pH 1.2 and pH 2.8. If thymol blue is…

A: The objective of the question is to determine the pH and nature (acidic, basic, or neutral) of a…

Q: If 20 ml of 0.1M NH4OH is added to 10 ml of 0.2M NH4Cl. What are the equilibrium concentrations of…

A: In Summary we will have:pH: 9.26Equilibrium Concentrations:[NH4OH] ≈ 0.067 M[NH4+] ≈ 0.067 M[OH-] =…

Q: What is a description of the salt that is used in a buffer solution? O from the conjugate base from…

A: buffer solution resist the change in pH of the solution,  when small amounts of strong acid or base…

Q: Explain why the pH does not change significantly when a small amount of an acid or base  is added to…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: The pH of an aqueous solution at 25°C was found to be 9.20. The pOH of this solution is The…

A: pH + pOH = 14  pOH = 14 - 9.2 = 4.8

Q: A general chemistry student mixes together a solution of HF with a solution of NaF. If the resulting…

A: Acidic buffer solution :- A mixture of weak acid and its salt with strong base is called acidic…

Q: Consider a solution that initially contains 0.40 mol fluoride anion and 0.30 mol of hydrogen…

A: Given information,         A solution that initially contains 0.40 mol fluoride anion and 0.30 mol…

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

A:

Q: You are given a 125 mL aqueous solution containing an unknown amount of NH4Cl salt. The solution has…

A: Given that, pH of solution =4.82  volume =125 ml =0.125 L  mass of NH4Cl =?

Q: A buffer solution is prepared by combining 0.898 moles of formic acid and 0.733 moles of sodium…

A: The buffer solution is prepared by mixing with 0.898 moles of formic acid and 0.733 moles of sodium…

Q: explain why the ph doesnt change significantly when a small amount of an acid or a base is added to…

A: pH doesn't change significantly when a small amount of an acid or a base is added to a solution that…

Q: Calculate the pH of the solution The K, value for HCN is 4.9 × 1 pH = Calculate the pH of the…

A:

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.21 M solution. The pH of the…

A:

Q: Calculate the pH of a solution that is 0.125M benzoic acid and 0.200M sodium benzoate, a salt whose…

A: Here, benzoic acid is a weak acid and sodium benzoate is a salt  Benzoate ion is the conjugate base…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.07 M solution. The pH of the…

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.