A buffer that contains 0.40 M base, B, and 0.25 M of its conjugate acid BH*, has a pH of 8.88. What is the pH after 0.0020 mol of HCl is added to 0.25 L of this solution?

Q: A buffer with a pH of 4.14 contains 0.31 M of sodium benzoate and 0.36 M of benzoic acid. What is…

A: Given data :

Q: Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.31 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵)…

A:

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: The Kb of ammonia is 1.76x10-5. What is the pH of a buffer which is prepared by combining 50.0mL of…

A: This question can be solved on the basis of the Handerson hasselbach equation which describes the…

Q: Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 1.09 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵)…

A:

Q: Consider a buffer made by adding 42.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)»NH (Kb = 5.4 x 10…

A: A buffer is made of a weak base and salt of that base. When an acid is added to the buffer, the base…

Q: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10⁻⁴) and 0.200 mol of NaF to…

A: HF    +          NaOH -----> NaF + H2O  Given  0.3 mol           0.040 mol…

Q: A buffer that contains 0.17 M of a base, B and 0.28 M of its conjugate acid BH+, has a pH of 8.9.…

A: A buffer is a solution that can resist a change in pH when small amount of base or alkali is added…

Q: Consider a buffer made by adding 48.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)2NH (Kb = 5.4 x…

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

Q: A buffer solution that is 0.458 M in HCN and 0.458 M in KCN has a pH of 9.40. The addition of 0.01…

A: The buffer solution consists of a weak acid (HCN) and the salt of weak acid and strong base (KCN).…

Q: A buffer containing 0.2000 M of acid, HA, and 0.1500 M of its conjugate base, A⁻, has a pH of 3.35.…

A:

Q: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10⁻⁴) and 0.200 mol of NaF to…

A:

Q: 2) How many grams of NaOH should be mixed with 5.4 g of oxalic acid (H,C.O.) and completed to 100 ml…

A:

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: How many grams of solid sodium cyanide should be added to 1.50 L of 0.172 M hydrocyanic acid…

A: The given data contains, Volume of HCN =1.50 LMolarity of HCN =0.172 MpH =8.570

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: A buffer that contains 0.55 M of the base, B, and 0.35 M of its conjugate acid, BH+, has a pH of…

A: Given: The concentration of base, [B] = 0.55 M The concentration of conjugate acid, [BH+] = 0.35 M…

Q: Consider a buffer made by adding 42.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)2NH (Kb = 5.4 x 10…

A: (CH3)2NH is a weak base and (CH3)2NH2I is its salt with a strong acid HI. Thus, the mixture is a…

Q: How many grams of solid sodium hypochlorite should be added to 2.00 L of a 9.04×10-2 M hypochlorous…

A: In the given question we have to calculate the gram of sodium hypochlorite to prepare the buffer…

Q: Calculate the pH of 1.00 L of the buffer 1.04 M CH3COONa/1.02 MCH₂COOH before and after the addition…

A: Using Henderson hasselbalch equation we can calculate the pH of buffer solutions.

Q: Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 1.09 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵)…

A:

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: How many grams of solid potassium hypochlorite should be added to 0.500 L of a 0.273 M hypochlorous…

A:

Q: A buffer that contains 0.110 M HY and 0.220 M Y⁻ has a pH of 8.77. What is the pH after 0.0015 mol…

A: Concentration of HY = 0.110 M Concentration of Y- = 0.220 M

Q: Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pKa=4.76) and 40.0…

A: pH = pKa + log [salt]/[acid] pKa = -log Ka Molarity = Number of moles of solute/volume of solution…

Q: A buffer that contains 0.40 M base, B, and 0.25 M of its con-jugate acid, BH⁺, has a pH of 8.88.…

A: Given data: Molarity of base B = 0.40 M Molarity of its conjugate acid BH+= 0.25 M pH = 8.88 Using…

Q: A buffer solution that is 0.471 M in HCN and 0.471 M in NaCN has a pH of 9.40. The addition of 0.01…

A:

Q: Consider a buffer made by adding 52.3 g of (CH3),NH2I to 250.0mL of 1.42 M (CH3)¿NH (Kb = 5.4 x…

A: The concentration or Molarity of salt is calculated by - M = w×1000/m×V Here, M = Molarity of Salt,…

Q: 4. A buffer is prepared containing 1.00 M acetic acid and 1.00 M sodium acetate. What is its pH?

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10⁻⁴) and 0.200 mol of NaF to…

A: Given-> Volume of buffer = 1.0 L Moles of HF = 0.300 mole  Moles of NaF = 0.200 mole Moles of HCl…

Q: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10⁻⁴) and 0.200 mol of NaF to…

A: Mole of NaOH = 0.07 Mol Mole of HF = 0.3 Mol Mol of NaF = 0.2 Mol

Q: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10⁻⁴) and 0.200 mol of NaF to…

A:

Q: A buffer solution that is 0.397 M in HCN and 0.397 M in KCN has a pH of 9.40. The addition of 0.01…

A: Given that, We have a buffer solution containing 0.397 (M) HCN and 0.397 (M) KCN. The buffer…

Q: Determine the resulting pH when 250 mL of 0.35 M HCI is mixed to a 800 mL buffer that has a…

A:

Q: Calculate the pH of a buffer that contains 0.390 M hydrazine, N2H4 (Kb = 1.3 × 10−6), with 0.264 M…

A: The H+ concentration of hydrogen ions that the given solution consists of determines the basic or…

Q: A buffer with a pH of 4.34 contains 0.33 M of sodium benzoate and 0.24 M of benzoic acid. What is…

A: To calculate the concentration of H3O+ after addition of HCl, we would calulate the pH of the buffer…

Q: How many grams of solid ammonium bromide should be added to 1.50 L of a 6.42x102 M ammonia solution…

A:

Q: A buffer with a pH of 4.31 contains 0.31 M of Sodium Oxalate Na2C2O4 and 0.24 M of Oxalic acid…

A: Value of pH is used to measure acidity or basicity of a solution. At room temperature, pH value lies…

Q: How many grams of solid potassium acetate should be added to 1.50 L of a 0.151 M acetic acid…

A:

Q: A buffer is prepared by mixing 204.0 mL of 0.452 M HCl and 0.500 L of 0.400 M sodium acetate…

A: Any particular buffer solution's pH can be derived by Henderson-Hasselbalch expression. Buffer…

Q: 4. Two RND Engineers were assigned to create buffer solutions for two separate product lines that…

A: We need to prepare buffer solutions and need to calculate pH and need to maintain it so that it…

Q: A buffer that contain 0.40 M of a base, B, and 0.25 M of its conjugate acid, BH+, has a pH of 8.88.…

A: Given:             Initial concentration of Base [B] = 0.40M   Initial concentration of Conjugate…

Q: Calculate the pH after the addition of 0.0050 mol of NaOH to the buffer in 9.1.4. (0.200 M NH4Cl -…

A:

Q: Consider a buffer made by adding 42.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)»NH (Kb = 5.4 x 10…

A: pH is a scale which is used to determine the acidity or basicity of a solution. pH = pKa + log…

Q: A buffer that contains 0.578 M base, B, and 0.299 M of its conjugate acid, BH*, has a pH of 9.09.…

A:

Q: Calculate the pH after the addition of 0.0050 mol of NaOH to the buffer in 9.1.4. (0.200 M NH4Cl -…

A:

Q: A buffer that contains 0.405 M base, B, and 0.296 M of its conjugate acid, BH", has a pH of 9.13.…

A: From Henderson Hasselbalch equation: pH=pKa+logconjugate baseacid Given, [B] is 0.405 M, [BH+] is…

Q: The Ka of hyperchlorous acid, HClO is 3.50 X 10-8. How many grams of NaClO (molar mass = 74.5…

A: 1- First calculate the concentration of NaClO :  Using the Henderson equation,  pH = pKa +…

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.