1. Calculate how much CH3COONa (Sodium Acetate Salt) to make 100mL of a 0.100M acetate buffer with a pH of 5.0

Q: When 25 .00 mL of 0.1098 M HCl in 40 mL of DI water is titrated against 0.09998 M NaOH, the pH…

A: The pH of a solution describes the acidity or basicity of the solution. If pH is greater than 7, it…

Q: You are making 100 mL of a 0.66M phosphoric acid buffer with a pH of 7.0. What is the concentration…

A:

Q: what volume of 0.10 M sodium acetate must be added to 20.0 ml of 0.20 M acetic acid to produce a…

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

Q: 1- Calculate the pH of 2 solution prepared by adding 25 ml of 0.IM of NAOH solu. to 30 ml of 0.2M of…

A: “Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: To make a common phosphate buffer using potassium hydrogen phosphate and potassium dihydrogen…

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

Q: Which pair of solutions forms a -5 buffer solution when equal volumes * ?of each are mixed 0.2M HCl…

A: Answer: option 2 : 0.4M CH3COOH and 0.2M NaOH will make a buffer solution when equal volume are…

Q: pH = 6.9 small can be neutralized can not be neutralized is not dissolved large Reset Help When…

A: Buffer solution — A solution which prevents change in pH on adding small amount of any acid or base…

Q: How to make 100 ml of buffer solution (ammonia - ammonium chloride) with pH = 10?

A: There may be many possibility to make buffer of pH =10 , Here only one possibility is discussed.

Q: Which of the following pairs would make a buffer? O HNO3 and NO2 O KBr and HBr NH3 and NH4*CI NaCl…

A: buffer : it is a mixture that resist change of pH by adding small amount of buffer solution. buffer…

Q: volume of 0.028 M NaOH must be added to 0.75 L of 0.0900 M HCl to achieve a pH of 9.00?

A: Total 2.445 L of 0.028 M NaOH solution is needed.

Q: Calculate the mass of KNO2 (85.10 g/mol) that must be added to 125 mL 0.220 M HNO2 to have a buffer…

A: Given: pH=4.0 Ka of HNO2.=4.5×10-4 Molarity of HNO2=0.220 M. The molar mass of KNO2=85.10 g/mol

Q: buffer

A:

Q: If a buffer solution is 0.160 M in a weak acid (K₁ = 1.9 × 10-5) and 0.450 M in its conjugate base,…

A: Given,  Concentration of weak acid = 0.160 M  Ka = 1.9 x 10-5  Concentration of Conjugate base =…

Q: You are making 100 mL of a 0.66M phosphoric acid buffer with a pH of 7.0. What is the concentration…

A: Here we have to determine the concentration of base component of phosphoric acid buffer needed to…

Q: Which acid would be best to use when preparing a buffer with a pH of 4.72? A list of Ka values can…

A:

Q: Q1// A buffer solution prepared by adding adequate amount of Acetic acid and Sodium acetate to…

A: Firstly we will calculate pH of buffer solution  CH3COOH - CH3COONa CH3COOH (aq) + H2O (l)⇌H3O+​…

Q: A buffer solution is 0.384 M in H2CO3 and 0.328 M in KHCO3. If Kal H2 CO3 is 4.2 × 10-7, what is the…

A: Answer 1 As we know the pH of acidic buffer solution is given by the formula pH = pKa +…

Q: Q1// A buffer solution prepared by adding adequate amount of Acetic acid and Sodium acetate to…

A:

Q: 85.0 mL of 0.20M HF (K, = 7.2 x 104)is titrated with 5.0 mL of 0.40 M NAOH. Calculate the pH at this…

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Q: Adding 100. ml of 0.100 M NaOH to 100. ml of 0.175 M NH4Cl, calculate the pH for the solution. (Ka…

A:

Q: You plan to make a buffer solution with sulfurous acid (H₂SO) and it undergoes dissociation reaction…

A: Henderson-Hasselbalch equation is used to prepare a buffer solution of desired pH: Desired pH is…

Q: You have a buffer composed of HCO3- and CO32-. Which ion represents the weak acid? and Which ion…

A:

Q: 4- A liter of solution contains 0.25 M HCOOH and 0.3 M HCOONA, calculate the pH of this solution.…

A:

Q: |Ka for formic acid is 1.7 x 10-4 at 25°C. A buffer is made by mixing 425 mL of 0.428 M formic acid,…

A: Given: Ka of formic acid = 1.7×10-4 Concentration of formic acid (M1) = 0.428 M Concentration of…

Q: 1_Determine the volume of concentrated ammonia and the weight of ammonium chloride needed to prepare…

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Q: Calculate the pH of a 0.100 M Na3PO4 solution. Find the mL of 0.40 M HClO4 that must be added to 100…

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Q: When a small amount of strong base is added to an ammonia/ammonium chloride buffer, what happens to…

A:

Q: 1. Calculate the pH of a solution after titrating 20.00 mL of 0.11 M nitric acid with 4.40 mL of…

A: Titration: It is an analytical technique that is used to determine the concentration of a solution…

Q: Consider a buffer solution comprised of HF and F. The K₂ of HF is 6.3 x 10-4. If the pH of the…

A: Given here, a buffer solution comprised of HF and F-. we are asked to  calculate the number of moles…

Q: Q1. In Part B of the lab, you are going to see how the pH of the buffer will change after adding…

A: Given ,

Q: The next 11 questions are related to the titration of 40.00 mL of a 0.0900 M acetic acid solution…

A:

Q: What volume of 0.028 M NaOH must be added to 0.75 L of0.0900 M HCl to achieve a pH of 9.00?

A: Given ,  Molarity of NaOH ( Mb ) = 0.028 M  Volume of NaOH ( Vb ) = ? Volume of HCl ( Va ) = 0.75 L…

Q: 1. When 50.00ml of 1.000M HCl is titrated with 0.750M NaOH, the pH increases. What volume of NaOH is…

A: Titration is the process that helps to determine the concentration of a substance reacting in a…

Q: How many grams of NaHCO3 should be mixed with 4.500 g of NaCO3 to produce 150.0 mL of buffer with a…

A: The given weight of Na2CO3 is 4.500 g. The molar mass of Na2CO3 is 105.98 g/mol. The formula to…

Q: 2. How many moles of HOCI should be present together with 0.50 mole of Ca(OCI)2 in a 1.00 L solution…

A: Step 1:Step 2:Step 3:Step 4:

Q: What is a buffer solution? What constitutes a buffer solution?

A: Ab buffer solution is a solution that consists of a mixture of weak acid along with its conjugate…

Q: Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25…

A:

Q: #4. What will be the pH if 125 ml 1.0 M HCI is mixed with 100 ml of 1.0 M NAOH?

A:

Q: You have 75.0 mL of 0.10 MHA. After adding 30.0 mL of 0.10 MNAOH, the pH is 5.70. What is the K.…

A: HA is a weak acid and NaOH is strong base, when NaOH is added it can not completely neutralize the…

Q: 4. Calculate the pH of a 1L solution containing 10 mL of 2 M acetic acid and 5 g of sodium acetate…

A:

Q: What is the pH ‘of a 100 ml 0.1M HCl solution after adding 90 ml

A: Answer: pH = 2.28  Solution:

Q: Calculate the pH of a solution that contains 0.10 M ammonium hydrochloride and 0.010 M HCl

A: GIVEN:- Calculate the pH of a solution that contains 0.10 M ammonium hydrochloride and 0.010 M HCl…

Q: What is the pH of buffer solution containing 0.25 M acetic acid and 0.4 M sodium acetate ?

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

Q: 4. If you titrate 100 mL of an unknown strong acid solution with 0.1 M NaOH, will the pH ever reach…

A: Acid base titration: In acid base titration a solution of known concentration  is added to a…

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.