What is the pH of a buffered solution that contains 0.25 M NHz and 0.22 M NH,CI?

Q: 2. A solution of 50.0 mL of 0.40 M NH3 is being titrated with a 0.40 M solution of the strong acid…

A: At half equivalence point concentration of conjugate acid and weak base becomes equal. Hence…

Q: A solution of 0.2 M HCl is mixed with 0.3 M NH4Cl.  Is this a buffer?

A:

Q: What must be the concentration of Ag* to just start precipitating 0.10M PO?0.10 M CI

A:

Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 8.0.

A: Given:   The pH value of Ni(OH)2 is 8.0. The value of Ksp is not given. Thus, so it is taken from…

Q: Calculate the pH of a buffer solution that is 0.339 M in NH3 (ammonia) and 0.143 M in NH4CI. pH =

A: Here we are required to find the pH of the buffer solution.

Q: Calculate the pH of a buffer that is 0.250 M in NaHCO3 and 0.280 M in Na2CO3.

A:

Q: Which of the following mixtures will result in a buffer solution? a. 0.1 M NH, and 0.1 M CUOH b. 0.1…

A: Buffer is a solution that resist the change in pH. Buffer is formed by a weak acid and its conjugate…

Q: What is the pH of a buffer solution that contains 20.0mL of 0.10M H2CO3 and 50.0mL of 0.10M NaHCO3?

A: We would use Henderson Hasselbalch equation to calculate the pH of buffer solution.

Q: What will be the pH of a buffer solution prepared from 0.20 mol NH3, 0.40 mol NH4NO3, and just…

A: Given : a buffer solution of weak base NH3 with its conjugate acid NH4NO3  Since moles =…

Q: A buffer solution is 0.486 M in NaH2PO4 and 0.394 M in Na, HPO4. If Ka for H2PO4¯ is 6.2 × 10¬8,…

A:

Q: An analytical chemist is titrating 117.3 mL of a 0.2700 M solution of butanoic acid (HC,H,CO, with a…

A:

Q: A 50.00 mL aliquot of 0.0100 M NH3 is titrated with 0.02136 M HCl. What is the pH of the solution at…

A:

Q: Calculate the pH of a buffer solution that is 0.496 M in C5H5N (pyridine) and 0.492 M in C5H5NHBr.…

A: GivenConcentration of the base pyridine, [C5H5N] =0.510MConcentration of the conjugate acid…

Q: 100.0mL of a 0.050M HNO2 solution is titrated with a 0.10M NaOH solution. a) What is the pH of the…

A: Given: Volume of HNO2 = 100 ml Concentration of HNO2 = 0.05 M Volume of NaOH = 10 ml  Concentration…

Q: A buffered solution is made by adding 80.0 g NH, Cl to 1.00 L of a 0.90-M solution of NH3. Calculate…

A:

Q: A buffered solution contains 0.50M H3CCO,H (acetic acid), which has a K. = 1.8 × 10-5, and 0.75M…

A: Buffer is a solution which resists the change in pH of a solution by the addition of acid or base.…

Q: A buffer solution is 0.080 M in lactic acid (Ka = 1.8 × 10−4) and 0.070 M in sodium lactate. The pH…

A: This is actually a buffer mixture of weak acid (lactic acid) and it's salt(sodium lactate).…

Q: A buffer solution is made that is 0.411 M in CH3COOH and 0.411 M in CH3CO0NA. (1) If K, for CH3COOH…

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

Q: determine the pH on the buffer of (NH4) 2SO4 and NH4OH

A: Buffer solutions are those, that can resist the pH change on the addition of some acidic or basic…

Q: A buffer solution is prepared by dissolving  1.300 g  of ammonium chloride (NH4Cl) into  100.00 mL…

A: Mass of ammonium chloride is 1.3 g. Molar mass of ammonium chloride is 53.491 g/mol.

Q: 6. Suppose you have a solution that was prepared by mixing equal amounts of nitric acid (HNO:) with…

A: In this question, we want to explain no more than two sentence that resulting solution is a buffer…

Q: A buffer solution is prepared by taking 0.25 moles of acetic acid (pKa = 4.76) and 0.400 moles of…

A: Given: Moles of acetic acid = 0.25 mol Moles of barium acetate = 0.400 mol Volume of solution =…

Q: A buffer solution is prepared by taking 0.400 moles of acetic acid (pKa = 4.76) and 0.250 moles of…

A: The Henderson Hasselbalch equation for acidic buffer solution is given as :

Q: 5. Calculate the pH of a buffer system containing 1.0 M CH,COOH and 1.0 M CH,COON..

A: 5. Given information,      1.0 M CH3COOH and 1.0 M CH3COONa

Q: (a) What is the pH of this buffer solution? (b) If 0.005 mol NaOH is added to 0.500L of this buffer…

A: pH can be calculated by using Henderson Hasselbalch equation  pOH = pkb + log ([salt]/[base]) pH =…

Q: 1. Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.O М СНЗСОONa. 2. What is the…

A: Given data,   Concentration of CH3COOH = 1.0M Concentration of CH3COONa = 1.0M…

Q: A buffer solution is prepared by dissolving 1.000 g of ammonium chloride (NH,CI) into 100.00 mL of a…

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: 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: What is the molar solubility of BaSO₄?

A: The solubility depends upon temperature and the Ksp value. The solubility is the ability of a…

Q: Calculate the pH of a buffer solution that contains 0.76 M NaH2PO4 and 0.28M Na2HPO4.   Calculate…

A: The equilibrium reaction can be represented as,

Q: A buffer is prepared by adding 35 mL of 0.100 M hypochlorous acid, HOCl, to 65 mL of 0.300 M…

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: A solution is made 1.1 * 10 - 3 M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches…

A: The reaction is – Zn2+ aq+ 4NH3aq ⇔Zn(NH3)42+aq

Q: Which hydroxide has the lowest molar solubility in H2O?

A: Ksp is know as the solubility product constant. The above mentioned question is explained below :

Q: Consider a buffer solution that contains 3.87 M KClO2 which has a Ka value of 0.011 and 5.69 M…

A: Answer: Buffer solution is the type of solution that resists the change in its pH on adding small…

Q: 4. The molar ratio between a weak acid and its base conjugate was (3:2). Calculate the Ka of the…

A: Hendrson hasselbalch equation will be use to determine Ka value

Q: the PH of sodium acetate/acetic acid buffer is 4.5 calculate the ratio of [CH3COOH]/[CH3COO^-]

A:

Q: (a) Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 M CH3COONa. (b) What is the…

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: Calculate the molar solubility of BaSO4 in a solution in which H3O+ is 0.5 M

A:

Q: Calculate the pH of the buffer system made up of 0.17 M NH3/0.47 M NH,CI.

A: Given : buffer solution of 0.17 M NH3 and 0.47 M NH4Cl  To calcxulate :- pH of  given buffer.

Q: Calculate the pH of a buffer solution that contains 0.79 M NaH2PO4 and 0.13M Na2HPO4   Calculate the…

A: The equilibrium reaction can be represented as,

Q: Calculate the molar solubility of Sn(OH)2 in a buffer solution containing equal concentrations of…

A:

Q: a. What is the pH of a buffer solution that is 0.12 M NH3 and 0.12 M NH4 +? К, for NH3 is 1.8 x 10-5…

A: The solution which resist the change in pH by addition of small amount of strong acid or a strong…

Q: A 1.00 L buffer solution is 0.125 M in HF and 0.125 M in NaF. Calculate the pH of the solution after…

A:

Q: a buffer is prepared by adding 115 mL of .30M NH3 to 135 mL fof .15 M NH4NO3. what is the pH of the…

A: A buffer is prepared by adding 115 mL of 0.30 M NH3 to 135 mL of 0.15 M NH4NO3. The pH of the final…

Q: 2.4. Consider a buffer solution that is 0.24 M NH3 and 0.20 M NH CI If 0.005 mol of NaOH is added to…

A: We would first Calculate initial pH of buffer solution. Then we need to calculate oH after adding…

Q: A buffer solution is prepared by taking 0.250 moles of acetic acid (pKa = 4.76) and 0.400 moles of…

A: From the Henderson-Hasselbalch equation:

Q: What is the pH of a buffer solution containing 1.25 M NH₃ and 0.78 M NH₄NO₃?

A: Given : Concentration of weak base NH3 = 1.25 M And concentration of conjugate acid salt of weak…

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.