What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.150 mol of KBrO in 2.0 L of solution?

Q: Calculate the pH of a solution that is 0.200 M in NH3 and 0.300 M in NH4Cl. Calculate the pH change…

A: Using Henderson-Hasselbalch equation: pH = pKa + log BaseAcid And, pOH = pKb + log AcidBase

Q: What is the pH of a buffer made from 0.580 mol of CH₃NH₂ (Kb = 4.4 × 10⁻⁴) and 0.180 mol of CH₃NH₃I?

A: Concentration of CH3NH2 = 0.580 Concentration of  CH₃NH₃I = 0.189 Kb = 4.4 × 10-4  pH = ?

Q: A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate.…

A: The pH of buffer solutions can be calculated with the help of Henderson-Hasselbalch equation. This…

Q: Consider the titration of a 60.0 mL of 0.291 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH. What…

A: The question is based on the concept of titrations. we have been given a weak Acid which is titrated…

Q: what is the ph of a buffer made from 0.080 mol of HCNO (Ka=3.5x10^-4) and 0.410 mol of NaCNO in 2.0…

A: In this question, we will determine the pH value of buffer solution which is made from the weak acid…

Q: How many grams of sodium hydroxide are needed to be added to 534 mL of 0.450 M HA solution to…

A:

Q: A buffer solution is made that is 0.372 M in HF and 0.372 M in NaF. If Ka for HF is 7.20 x 10-4,…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

Q: How many grams of NaOH must be added to 1.50 L of a 0.400 M solution of oxoacetic acid (HCOCO2H) to…

A:

Q: For 240.0 mL of a buffer solution that is 0.195 MM in HCHO2 and 0.295 M in KCHO2, calculate the…

A:

Q: 45.0 mL of a buffer solution contains 0.20 M CH₂COOH and 0.25 M CH₂COONa. What is the pH of the…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.  It…

Q: A buffer solution was prepared that contained 0.60 M hydrogen fluoride, HF (Ka = 7.2 x 104) and…

A: An aqueous solution efficient to withstand the pH changes and comprising weak acid/base combined…

Q: Let’s build a buffer using hypobromous acid (HBrO, Ka = 2.3×10−9) and hypobromite ion (BrO−). If…

A: Given: The concentration of hypobromous acid [HBrO]=0.100 M Ka=2.3×10−9 pKa= -log (2.3×10−9)…

Q: The titration curve as shown is for the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH.…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: Given : Mass of CH3COONa = 1.000 g Volume of acetic acid solution = 100.00 mL = 0.100 L…

Q: How many grams of sodium hypochlorite, NaCIO, need to be added to 227 mL of a 0.185 M solution of…

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.