the solution of 2.50 L of a 0.250M CH3CO2H has a pH of 4.20, what is the pH if you add 20.0 mL of 0.10M HCL? For CH3CO2H the Ka= 1.76 X10^-5

Q: Calculate the pH of a solution made by adding 0.114 g of solid NaOH to 475 mL of 0.150 M HNO2 (Ka =…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

Q: A student has a sample of 0.50 M lactic acid (HC3H5O3). She adds 10 mL of this solution to 40 mL of…

A: Given : Concentration of lactic acid = 0.50 M Volume of lactic acid solution used = 10 mL = 0.010 L…

Q: Calculate the pH when 29.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: The values of K a for hydrozoic acid ( HN 3) and hypobromous acid (HBrO) are given below. HN3 Ka =…

A: Given: HN3 Ka = 1.9 × 10-5 HBrO Ka = 2.0 × 10-9

Q: Given Ka for HNO2 = 5.0 * 10 ^ - 4 1. What is the pH after the reaction of 30.0 mL of 0.25 M HBr…

A: Q1) According to the law of equivalence, an acid exactly neutralizes the same number of equivalents…

Q: What is the pH for a 400 ml solution of 1.6 M Benzoic Acid if you added 175 grams of conjugate base…

A: The solution is given below -

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 36.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Buffer Mixture is defined as an Aqueous solution which contains weak acid or weak base with its…

Q: What is the pH of the resulting solution if 45.00 mL of 0.10 M acetic acid is added to 10.00 mL of…

A: Given data contains, Volume of acetic acid is 45.00mL. Molarity of acetic acid is 0.10 M. Volume of…

Q: t is the pH of a 0. M solutI 350 M solution of NaOH is added? The K, of HA is 4.3 x 10-4.

A: We have to tell which option is correct from given choices of options by telling what is the pH of…

Q: One of the buffers that contributes to pH stability in human blood is carbonic acid (H2CO3).…

A: If the pH of the blood increases the buffer will act in such a way that reduces the pH. It is the…

Q: What is the pH of a solution of 100 mL of 0.025 M HBr and 100 mL of 0.10 M NaF? (HF Ka= 7.2 x 10-4)

A: Given Volume of HBr solution = 100 mLConcentration of HBr solution = 0.025 MVolume of NaF solution =…

Q: What

A: Dear student I have given answer to your question in the image format.

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 42.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: ph of a 30.0 ml sample of 0.1 M HOAc is 3.22, what's the equilibrium [H+] and the Ka value?

A: Given :- pH is 3.22 of a 30.0 mL sample of 0.1 M HOAc. To calculate [H+] & Ka value.  Now, HOAc…

Q: A 13.6 mL solution of 0.100 mol L-1 CH3COOH is titrated using 0.150 mol L-1 NaOH. What is the pH of…

A:

Q: What is the pH of a solution

A:

Q: What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH 3CO 2H with 30.00 mL of 0.030…

A: The question is based on the concept of titrations.   we are titrating  a weak acetic acid with a…

Q: Write the basic equilibrium equation for BrO₃⁻.

A: NOTE: Since you have asked multiple question, we will solve the first question for you. If you want…

Q: Calculate the pH of a solution that contains 3.25 M HCN (K a = 6.2 x 10 -10 ), 1.00 M NaOH and 1.50…

A: Detail

Q: Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: Calculate the K₂ for a monoprotic acid, HX, if a 0.100000 M solution has a pH of 3.333. The data is…

A: The given reaction is : HX     +     H2O      ⇔       X-     +     H3O+ The answer is as follows:

Q: Calculate the pH of a solution made by adding 0.123 g of solid NaOH to 275 mL of 0.350 M HNO2 (Ka =…

A:

Q: Calculate the pH of a solution at the equivalence point when 200.0 mL of a 0.20 M solution of Lactic…

A:

Q: What is the pH of the solution containing 0.1M sodium formate (NaHCOO) and 0.05M formic acid…

A: Required data to determine the pH of buffer solution using Henderson equation.

Q: A student has a sample of 0.50 M lactic acid (HC 3H5O 3). She adds 10 mL of this solution to 40 mL…

A: The objective of the question is to write a chemical reaction for the dissociation of lactic acid in…

Q: Calculate the pH when 31.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: KOH + HOBr = KOBr + H2O Moles of HBrO = Molarity x volume in…

Q: Calculate the Ka of a weak monoprotic acid if a 0.10 M aqueous solution of the acid has a [H+] of…

A: An acid dissociation constant can be defined as the quantitative measure that is used to describe…

Q: Calculate the pH when 22.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: What is the pH of the solution when 25.00 mL of 0.300 M nicotinic acid (HNic) is titrated with a…

A: pH can be calculated by using Henderson Hasselbalch equation pH = pka + log([salt]/[weak acid])

Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…

A:

Q: pH

A:

Q: a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the…

A: The pH of this buffer solution can be calculated by using Handersson-Hesselbalch equation-

Q: An analytic chemist is titrating 65.9 mL od 0.4200 M solution of piperidine (C6N10NH) with a 0.8800…

A: First calculate the number of moles for both given base and acid. Then use that moles to find out…

Q: Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 1.5 × 10−6) is titrated with 0.10 M…

A:

Q: None

A: (b) Addition of 3.00 mL of 0.500 M NaOH to 30.0 mL of buffer:Given pH: 8.13(c) Addition of 15.0 mL…

Q: What is the pH of a solution containing a mixture of 0.050 M HC2H3O2 and 0.025 M NaC2H3O2?  (Ka =…

A: Given: [HC2H3O2]=0.050 M [NaC2H3O2]=0.025 M Ka = 1.8 × 10-5 pKa=-log (1.8 × 10-5) pKa=4.745

Q: What is the pH when 20.0 mL of 1.00 M NaOH has been added to 25.0 mL of 1.00 M CH3COOH…

A: The pKa of the acetic acid is equal to –log(Ka) = 5 – log(1.8) = 4.75 Number of moles of acetic acid…

Q: What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to…

A:

Q: Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5. FW(propanoic acid) = 74.08 g/mol; FW(calcium…

A: Buffers are generally good over the range pH = pKa ± 1. For example, the acetate buffer would be…

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.