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

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: 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: A solution contains 0.119 M ammonium chloride and 0.126 M ammonia. The pH of this solution is

A: The given data contains, Molarity of ammonium chloride = 0.119 M. Molarity of ammonia = 0.126 M pKb…

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 solution contains 0.437 M sodium acetate and 0.397 M acetic acid. The pH of this solution is

A: Given : concentration of sodium acetate = 0.437 M  Concentration of acetic acid = 0.397 M  To…

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

A: In buffer solution  salt and acid concentration given than ph eaisly calculated.

Q: A solution contains 6.30x102 M potassium nitrite and 0.345 M nitrous acid. The pH of this solution…

A: Given-> Concentration ofpotassium nitrite(KNO2)=6.30 ×10-2M Concentration of nitrous acid (HNO2)…

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

A:

Q: contains

A: For calculating the pH, we can used Hinderson equation,  pH = pKa + log( [salt] / [ acid ] )  Where…

Q: A solution contains 0.392 M NH¸I and 0.134 M ammonia. The pH of this solution is

A:

Q: A solution contains 0.160 M sodium cyanide and 0.255 M hydrocyanic acid. The pH of this solution is

A:

Q: A solution is 0.0500 M in NH4Cl and 0.0300 M in NH3. Calculate its OH- concentration and its pH.

A:

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

A:

Q: An aqueous solution of 0.1 M hydrochloric acid with a volume of 200 milliliters is mixed with 100 mL…

A: Moles of HCl taken = molarity of HCl X volume of HCl solution taken in L Since molarity of HCl = 0.1…

Q: A solution contains 0.297 M ammonium chloride and 0.246 M ammonia. The pH of this solution is

A:

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 solution contains 0.119 M sodium cyanide and 7.32×10-2 M hydrocyanic acid. The pH of this…

A:

Q: A solution contains 0.171 M ammonium iodide and 0.339 M ammonia. The pH of this solution is

A:

Q: A solution contains 0.483 M potassium cyanide and 8.14x10-2 M hydrocyanic acid. The pH of this…

A:

Q: The compound methylamine is a weak base like ammonia. A solution contains 9.91x10-2 M CH3NH3+ and…

A:

Q: A solution contains 0.252 M sodium nitrite and 0.179 M nitrous acid. The pH of this solution is

A:

Q: An aqueous solution contains 0.411 M Na,HPO4 and 0.436 M H,PO4. The pH of this solution is

A:

Q: A solution contains 0.219 M potassium nitrite and 0.218 M nitrous acid. The pH of this solution is

A:

Q: A solution contains 0.145 M ammonium chloride and 0.108 M ammonia. The pH of this solution is

A:

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: A solution contains 0.354 M potassium cyanide and 0.401 M hydrocyanic acid. The pH of this solution…

A: The given problem can be solved by using Henderson-Hasselbalch equation as; pH = pKa + log SaltAcid…

Q: A solution contains 0.230 M sodium hypochlorite and 0.196 M hypochlorous acid. The pH of this…

A: The equation which gives the relationship between pH and pOH of a solution, pK_a and pK_b and ratio…

Q: A solution contains 0.237 M sodium fluoride and 0.352 M hydrofluoric acid. The pH of this solution…

A:

Q: A solution contains 0.280 M ammonium iodide and 0.161 M ammonia. The pH of this solution is

A: Given: Ammonium iodide [NH4I]= 0.280 M Ammonia [NH3] = 0.161 M pH = ? The given solution is a buffer…

Q: A solution contains 0.155 M potassium cyanide and 0.171 M hydrocyanic acid. The pH of this solution…

A:

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

A:

Q: contains

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: The pH of this solution

A:

Q: A solution contains 6.88×102 M sodium fluoride and 0.129 M hydrofluoric acid. The pH of this…

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.