Calculate the K sp for hydroxide if the solubility of Sr(OH) 2 in pure water is 1.42 × 10 1 g/L.

Q: A chemistry graduate student is given 100. mL of a 0.70M chlorous acid (HC1O₂) solution. Chlorous…

A:

Q: A chemistry graduate student is given 250. mL of a 0.70M hydrocyanic acid (HCN) solution.…

A:

Q: A chemistry graduate student is given 100. mL of a 1.70M hydrocyanic acid (HCN) solution.…

A: We have to calculate the mass of NaCN for the buffer solution

Q: Calculate the solubility of Mg(OH)2 in 0.50 M NH4Cl.

A: The reaction of Magnesium hydroxide in NH4Cl is because of ammonium ion which reacts with OH- of…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: Here we have a buffer solution which has:Concentration of NH4Cl/NH4+ = 0.181 MConcentration of NH3 =…

Q: You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 M sodium…

A: We have to predict the pH of final buffer solution.

Q: A chemistry graduate student is given 300. mL of a 0.20M nitrous acid (HNO,) solution. Nitrous acid…

A:

Q: In an alkalinity titration of a 100.0 mL sample of water from a hot spring, 2.56 mL of a 0.0315 M…

A: At the first equivalence point, the reaction can be given as follows: HCl+CO32-→HCO3-+Cl- From the…

Q: Calculate the solubility of aluminum hydroxide, Al(OH)3, in a solution buffered at pH 11.00.

A: Solubility product, Ksp of Al(OH)3 is 1.9×10-33. pH of the solution = 11.00 pOH of the solution = 14…

Q: Calculating the composition of a buffer of a given pH A chemistry graduate student is given 125. mL…

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Q: What is the molar solubility of lead chloride (PbCl2) if the solubility is 1.1 x 10^-2 g/L.

A: Atomic mass of Cl = 35.453 g/mol Atomic mass of Pb = 207.2 g/mol Molar mass of PbCl2  = (207.2 +…

Q: The solubility product constant of Cu(OH)2 and Mg(OH)2 are 1.6 × 10-9 and 6.0 × 10-12, respectively.…

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Q: Determine the molar solubility of BaF 2 in pure water. K sp for BaF 2 = 2.45 x 10 -6. 2.45 x 10 -6…

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Q: A chemistry graduate student is given 125. mL of a 1.30M dimethylamine ((CH,) NH) solution.…

A: Buffer solution:  It is a special type of mixture of a weak acid or a weak base and its conjugate…

Q: A chemist creates 0.375 L of a 0.18 M acetic acid (CH3COOH) and 0.29 M sodium acetate (CH3COONa)…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a buffer…

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.