What is the pH of a buffer that contains 0.20 M CH 3COOH and 0.15 M NaCH 3COO?

Q: 1. Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 М СНЗСООNa.

A: According to guidelines i can answer only 1st question

Q: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10 4) and 0.410 mol of NaCNO in…

A: Henderson's Equation:- This equation gives the pH of a buffer solution.  The number of moles of salt…

Q: If (HSO, ] = .3 M, what [SO,² ] is needed to make a buffer of pH 2.6?

A:

Q: A buffer contains 0.025 mol of lactic acid (pK, = 3.86) and 0.060 mol of sodium lactate per liter.…

A: Dear student, As you have asked multiple question but according to guidelines we will answer the…

Q: 5) Part 2 Calculate the pH at the stoichiometric point when 25 mL of 0.091 M nitric acid is titrated…

A: The given acid (nitric acid) and base (NaOH) is strong acid and strong base respectively.

Q: Why the concentrations of buffer components must be high to minimize the change in pH from addition…

A: A buffer solution or pH buffer  is an aqueous solution consisting of a mixture of a weak acid and…

Q: What is the pH of a buffer made from 0.190 mol of HCNO (Ka = 3.5 x 10 4) and 0.410 mol of NaCNO in…

A: A buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its…

Q: What is the pH of a buffer that contains 0.20 M CH 3COOH and 0.20 M NaCH 3COO?

A: A buffer solution is formed by the mixture of a weak acid and its conjugate base or a weak base and…

Q: You have a 0.500 L buffer solution composed of 0.47  M formic acid (HCOOH, Ka = 1.77 x 10¯4) and…

A: The acid ionization constant for acid is 1.77×10 -4.

Q: Calculate the pH of a buffer that was prepared by mixing 90 mL of a 0.01M aqueous hydrocyanic acid…

A: HCN is a weak acid. In presence of base it produces it's conjugate base and form buffer solution.…

Q: A buffer is made by dissolving 14.4 g of sodium dihydrogen phosphate, NaH2PO4, and 22.5 g of…

A: Given an acidic buffer solution. Amount of weak acid sodium dihydrogen phosphate NaH2PO4 is…

Q: Even though Ca(OH)2 is an inexpensive base, its limited solubility restricts its use. What is the pH…

A: The dissociation reaction of Ca(OH)2 can be written as follows,

Q: At 25 degrees Celsius, what is the pH of a buffer that contains 0.100 M dimethylammonium chloride…

A: dimethyl amine has pKa = 3.27

Q: A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this…

A:

Q: A buffer solution is made up of 0.90 M formic acid and 0.90 M sodium formate. The formic acid has a…

A: Given : Concentration of formic acid = 0.90 M Concentration of sodium formate = 0.90 M Comcentration…

Q: What is the pH of a buffer made from 0.350 mol of HBRO (Ка 3 (Ka = 2.5 x 10°) and 0.080 mol of KBRO…

A: Given : Moles of HBrO = 0.350 mol. Moles of KBrO = 0.080 mol. Ka of HBrO = 2.5 X 10-9  And volume of…

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

A:

Q: Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.2 M CH3COONa.

A: Ka for acid = 1.8 x 10-5  [CH3COOH] = 1.0 M [CH3COONa] = 1.2 M  PH = ?

Q: What is the molar solubility of Pb(OH)2 in a 0.138-M solution of CH3NH2?

A: Given: Concentration of CH3NH3+ solution = 0.138M The reaction of base with water is as follows,

Q: Consider the following reaction:   CH_3COOH(aq)+OH^-(aq)===>CH_3COO^-(aq)+H_2O(l) How much 5.70 M…

A: Answer: volume of NaOH added is 1 mL (approx).

Q: Calculate the change in pH when 0.0017 mol of HNO3 is added to 0.100 L of a buffer solution that is…

A: Answer: In this question we have to calculate the pH of the buffer solution before and after the…

Q: What is the pH of a buffer made from 0.140 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

A:

Q: Calculate the molar solubility of Al(OH)3 in a buffer solution with 0.100 M NH3 and 0.400 M NH4+.

A: Base dissociation constant Kb for ammonia is 1.8×10-5. NH3aq+H2Ol⇔NH4++OH- Kb=NH4+OH-NH3

Q: Consider a buffer made by adding 132.8 g of NaC,H;O2 to 300.0 mL of 1.31 M HC,H;O2 (Ka = 6.3 x 105)…

A:

Q: 2. There is a phosphate buffer with 0.1 M of NaH₂PO4 0.1 M of Na₂HPO4. Calculate pH of buffer…

A: A buffer solution is a combination of two solutions - a weak acid solution and the salt of its…

Q: A buffer solution contains 0.11 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L What…

A: We need to find pH of given solutions

Q: What is the pH for a buffer made of 0.214 MNH 3 and 0.107 MNH 4 Cl ? K b for NH 3 is 1.8 * 10 ^ - 5…

A: Given data is as follows: The concentration of NH3 = 0.214 M The concentration of NH4Cl = 0.107 M…

Q: A buffered solution containing 0.400 M aniline C6H5NH2 and 0.200 M aniline hydrochloride, C6H5NH3Cl…

A: pH is used to determine the concentration of hydronium ion .

Q: 2. How many grams of hydrofluoric acid, HF, should you add to a 1.65 L of a 2.65 M sodium fluoride…

A:

Q: 2. There is a phosphate buffer with 0.1 M of NaH2PO4 0.1 M of Na2HPO4. Calculate pH of buffer…

A: pH of a buffer solution can be calculated using H-H equation.

Q: An acetic acid buffer contains 0.6 M CH3COOH and 0.6 M CH3COONA. (CH3COOH has a K, 1.76 x 105.) What…

A: Given- Concentration of CH3COOH= 0.6M Concentration of CH3COONa= 0.6M Ka of CH3COOH=1.76 ×10 -5…

Q: 1. What is the pH of a buffer that contains 0.15 M CH,COOH and 0.10 M NACH,COO (K, = 1.8 x 10 )?

A: 1) Given, Concentration of CH3COOH solution = 0.15 M [CH3COOH] = 0.15 M Concentration of NaCH3COO…

Q: What is the pH of a buffer that is 0.12 M HNO2 and 0.16 M NANO2 and the pKa is 3.35?

A:

Q: What is the pH of the buffer 0.1 M Na2HPO4/0.15 M KH2PO4?

A:

Q: Describe the effect of pH on the solubility of Fe(OH)3

A: A reaction is said to be in equilibrium if the rate of the forward reaction is equal to the rate of…

Q: What is the molar solubility of Fe(OH)3?

A: Answer :-  Molar solubility of Fe(OH)3 = 9.95 × 10-11 (M)

Q: What is the pH of the solution after the addition of 0.10 mol of NaOH to a 1.00 L buffer solution…

A: Given,  Number of moles of NaOH added = 0.10 mol  Volume of the buffer = 1.00 L  Molarity of HCN =…

Q: A 50.0 mL solution of 0.150 M acetic acid (CH3 COOH) is titrated with 0.150 M NaOH. What is the pH…

A: Final answer : 4.921

Q: What is the pH of the buffer 0.10 M Na2HPO4/0.15 M KH2PO4? Ka = 6.17 x 10-8

A: The objective of the question  is to calculate the pH of the buffer solution where the buffer…

Q: What is the pH of a buffer system that is 0.25 M in NH3 and 0.26 M in NHẠCI? Kb NH3 = 1.8 x 105

A: To determine pH of buffer solution Henderson- Hasselbalch equation can be used. Given solution is…

Q: If you wanted to create a buffer with a pH - 3.2, what substances would you choose to make the…

A:

Q: What is the pH of a buffer made from 0.200 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

A:

Q: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

A: Henderson's equation for the calculation of buffer solution consisting of a weak acid and salt 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: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: Calculate the pH of the 0.30 M NH3/ 0.36 M NH4C1 buffer system. What is the pH after addition of 20…

A: A buffer is a solution which resist change in pH and obtained when a weak acid and the salt of its…

Q: A chlorous acid buffer containing 0.75 mol of HClO2(aq) and 0.75 mol of NaClO2(aq) in 1.00 L has a…

A:

Q: A certain weak acid, HA, with a K. value of 5.61 x 10-6, is titrated with NaOH.

A:

Q: What is the pH of a buffer that consists of 0.412 M methylamine CH3NH2 and 0.219 M methylammonium…

A:

Q: What is the pH of a buffer composed of 0.45 M C5H10NH and 0.65 M [C5H10NH2]Cl?

A: Formula for calculating pOH of a solution consisting of a weak base and its salt with a strong acid:…

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.