A buffer solution is made from 0.031 M Na2HPO4  and 0.069 NaH2PO4 . What is the pH of that solution after the addition of 1mL of 15M HCl? pKa is 6.86.

Q: A 50.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HBr. What is the most likely pH of the…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: Carbonic acid (H2CO3) is a weak diprotic acid with a first ionization constant, Ka1 = 4.2 x 10–7.…

A: H2CO3  → H+ + HCO3-  It is given that,Ka1 = 4.2x10-7   pKa = -log10 Ka[H2CO3] = [HCO3–] = 0.100 M…

Q: A buffer is created by dissolving 0.303 moles of lactic acid and 0.197 moles of sodium lactate in…

A:

Q: Calculate the pH of a solution that is 0.45 M CH3COOH and 0.75 M NaCH3COO. Sodium acetate/acetic…

A: Buffer is a solution which consists of a weak acid and it's conjugate base or weak base and it's…

Q: how many mols NaC2H2ClO2 must be added to 1.00 L of 0.25 M HC2H2ClO2 to prepare a buffer with pH =…

A: Buffer solution are those solution whose pH remains constant even on addition of strong acid or base…

Q: What is the pH of a buffer prepared by mixing 20.0 g of ethylamine, CH3CH2NH2, and 20.0 g of…

A: Given -> Weight of CH3CH2NH2 = 20.0 gm  Weight of CH3CH2NH3Cl = 20.0 gm Volume= 2.00 L

Q: Suppose you have a buffer, comprised of 0.350 mol of weak base and 0.250 mol of weak acid. Ifthe pH…

A: The of a buffer solution can be calculated using Henderson Hasselbalch Equation written as follows:…

Q: The p?apKa of hypochlorous acid is 7.5307.530. A 54.054.0 mL solution of 0.1190.119 M sodium…

A:

Q: A buffer is made up of 15.0 ml of 0.1 M HC,H,02 and 15.0 ml of 0.1 MNa CH,O, The solution is diluted…

A:

Q: How many grams of solid potassium hypobromite, KBrO must be added to 200.0 ml of 0.100M hypobromous…

A:

Q: A buffer is composed of 0.200 M (CH3)₂NH (K₁ = 5.9 × 104) and 0.250 M (CH3)2NH₂NO3. What is the pH…

A: Given,molarity of (CH3)2NH = 0.200 Mmolarity of (CH3)2NH2NO3 = 0.250 MKb of (CH3)2NH = 5.9 x…

Q: 15.0 mL of a buffer is made by mixing 10.0 mL of 0.10 M HF and 5.0 mL of 0.10 M NaOH solution. What…

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

Q: A solution is made by dissolving 0.1283 g of the acid form of the buffer TRIS (molecular mass =…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: What is the pH of a buffer

A: Buffer is a solution of weak acid and base. the pH of buffer can not changes with addition or acid…

Q: NH4

A: Given: Ammonia buffer solution: M1 =  0.25 M [NH4+] M2   = 0.22 M [NH3] pKa of NH4+ = 9.24

Q: You are working in a lab and someone has just handed you a beaker filled with 110 ml of a mysterious…

A: pH of a buffer is calculated using Hasselbach Henderson equation: pH =pKa+log([Conjugate…

Q: A buffer is prepared by mixing 48.2 mL of 0.196  M NaOH with 144.3  mL of 0.231 M acetic acid. What…

A: The objective of this question is to calculate the pH of a buffer solution after the addition of a…

Q: An ammonia buffer solution contains 0.20 M NH4+NH4+ and 0.21 M NH3NH3 . The pKa of ammonium is…

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

Q: what is the pH after adding 0.006 mol HCl to 0.3L of a buffer solution that is 0.250M HC2H3O2 and…

A:

Q: In a beaker, 16 mL of 0.60 M acetic acid is combined witu 4 mL of 0.60 M sodium acetate. Using the…

A: Given: Ionisation constant Ka = 1.8×10-5 Concentration of acetic acid = [HC2H3O2] = 0.60 M…

Q: A 1.49 L buffer solution consists of 0.142 M butanoic acid and 0.286 M sodium butanoate. Calculate…

A: Given: Volume of buffer solution = 1.49 L The concentration of butanoic acid, (HA) = 0.142 M…

Q: A 100mL sample of 0.20M HF is titrated with 0.10M KOH. What is the pH of the solution after the…

A: HF is a weak monoprotic acid with Ka = 3.5*10-4  KOH is a strong monoacidic base.

Q: A buffer is prepared by mixing 48.2 mL of 0.196  M NaOH with 144.3  mL of 0.231 M acetic acid. What…

A: The objective of this question is to calculate the pH of a buffer solution prepared by mixing a…

Q: 25 mL of a 0.0268 M solution of an unknown monoprotic acid was titrated with 0.0633 M NaOH solution.…

A: Given: Volume of monoprotic acid (assuming HA) = 25 mL = 0.025 L                            (since 1…

Q: The pKa of acetic acid is 4.74. What is the pH of a buffer solution that is prepared from 0.010 M…

A: Buffer solution have tendency to resist pH change on addition of small amount of strong acid or…

Q: A buffer solution is prepared by mixing together 29.00 mL of 0.15 mol L1 HA (a monoprotic weak acid…

A:

Q: What is the pH of a nitrous acid/nitrite buffer that consists of 0.15 M HNO2 and 0.65 M LiNO2? What…

A: First calculate the pH.  Then calculate the pH of new solution.

Q: Calculate the pH of a bicarbonate buffer that is composed of a solution that is 0.5 M sodium…

A: To calculate the pH of a bicarbonate buffer solution, you can use the Henderson-Hasselbalch…

Q: A buffer is prepared using 0.15 M HF and 0.15 M NaF. What is the pH of this buffer? pKa for HF is…

A: Given :-   [HF] = 0.15 M  [NaF] = 0.15 M  pKa for HF = 3.1  To calculate :-  pH of buffer

Q: if 0.1L of 0.1M NaOH is added to 0.9 l of 0.50 M acetate buffer at pH 4.76 what is the resultant PH?…

A: Answer: An acidic buffer solution is given to us and we have to find out the pH of the new buffer…

Q: A chemistry graduate student is given 300. mL of a 0.50M dimethylamine ((CH3)2NH) solution.…

A: ⏹️ Approach to solving the question: Here is a step-by-step approach to solving this problem: 1.…

Q: A buffer solution is created containing 3.25 M acetic acid and 0.550 M sodium acetate. The Ka of…

A: Given :-  [CH3COOH] = 3.25 M  [CH3COONa] = 0.550 M  Ka for acetic acid = 1.77 x 10-5  To calculate…

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.