You are conducting a biochemical experiment with an enzyme that has optimal activity at pH = 10.50. You decide to use carbonate (pKa1 = 6.38, pKa2 = 10.30) as the buffer to keep the pH stable throughout the enzymatic reaction. (Recall that the formula for carbonic acid is H2CO3.) You prepare a 0.6 M solution of carbonate buffer at pH = 10.50. Calculate the concentrations of the major carbonate species

Q: Calculate the pH of a blood plasma sample with a total CO, concentration of 25.7 mM and bicarbonate…

A: Given,The total concentration of CO2 is 25.7 mM.The concentration of bicarbonate is 24.4 mM.The pKa…

Q: The value of K, for hydroxylamine, NH,OH, is 9.10×10-9. Write the equation for the reaction that…

A:

Q: The value of K for methylamine, CH3NH₂, is 4.20x10-4. Write the equation for the reaction that goes…

A: Given, Kb(for methyl amine ) = 4.20×10-4

Q: 6. At 25.0°C, 65.0 mL of 0.784 M ascorbic acid, HC6H7O6 was mixed with 45.0 mL of 0.371 M KOH. Ka =…

A: We have calculate pH of the given solution

Q: 1) Calculate the pH of a solution prepared by dissolving 2.20 g of sodium acetate, CHCOONA, in 78.0…

A: Given: mass of sodium acetate=2.20 gvolume of acetic acid=78.0 mLmolarity=0.10 MKa=1.75×10-5 To…

Q: A buffer solution is prepared which is 0.260 M both in lactic acid (CH3CHOHCO2H) and in sodium…

A: Given,Molarity of lactic acid ( CH3CHOHCO2H ) = 0.260 MMolarity of sodium lactate ( CH3CHOHCO2Na ) =…

Q: You are studying an unusual enzyme that produces hydronium ions (H3O+) during the course of the…

A: This question is from ionic equilibrium. We will figure out it answer with proper explanation.

Q: 1,2-Dichloroethane is a volatile organic compound that was once added to gasoline along with the…

A: A.    Let the concentration of 1,2-Dicholoroethane  = C mg/m3 the carcinogenic risk (R) = CDL ×SF…

Q: A group of students were able to isolate a novel amylase from the saliva of a pig found in Country…

A: Given the desired pH = 7.4  We can find the most suitable buffer based on the Henderson equation.

Q: The ionization constant (K») of aniline (CsHsNH2) is 2.35 x 10-5, If 7.285 grams of aniline is…

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

Q: A chemistry graduate student is given 300. mL of a 1.70M trimethylamine ((CH3), N) solution.…

A:

Q: using the equation below and the principle of le chatelier explain how blood pH would be influenced…

A: pH of solution will be defined by the shifting of equilibrium position.

Q: Choose the acid below that would make the most effective buffer for a solution to maintain a pH of…

A:

Q: What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid…

A: We have to predict the pH of buffer solution.

Q: In the laboratory, a general chemistry student measured the pH of a 0.474 M aqueous solution of…

A:

Q: A compound has two carboxyls and one aminium group. The pKas of the groups are 1.9, 4.2, and 9.3,…

A:

Q: An analytical chemist is titrating 176.4 mL of a 0.2800M solution of trimethylamine ((CH3),N) with a…

A: Molarity of trimethylamine = 0.2800 mol/LMolarity of HNO3 = 0.7000 mol/LpKb = 4.19

Q: Both functional groups of salicylic acid ionize in water, with Ka = 1.0 × 10^-3 for -CO2H group and…

A: Given: Ka for –CO2H group = 1.0 x 10-3 Ka for –OH group     = 4.2 x 10-13 Solubility of salicylic…

Q: a) Write the chemical reactions whose equilibrium constants are Kb and Ka for imidazole and…

A: Acid dissociation constant, Ka is also known as the acidity constant. or acid ionization constant.…

Q: Draw the structure of the principal chemical form(s) that determines pH when the following compounds…

A: Acid are proton donors whereas bases are proton acceptors. Weak acids do not dissociate completely…

Q: Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer…

A: Given,Weak base in the buffer solution : PyridineConcentration of the salt solution = 0.62 MThe…

Q: An analytical chemist is titrating 112.7 mL of a 0.6400M solution of ethylamine (C₂H5NH₂) with a…

A: Given, Molarity of the ethylamine C2H5NH2 = 0.6400 M = 0.6400 mole/L The volume of the ethylamine…

Q: An analytical chemist is titrating 165.1 mL of a 0.8800M solution of diethylamine (C,Hs) NH) with a…

A:

Q: For a weak acid, when does the pH equal the pKa?

A: Answer: For this we need to know Henderson-Hasselbalch equation . Explanation:…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

A:

Q: A chemist titrates 80.0 mL of a 0.4857 M cyanic acid (HCNO) solution with 0.8029 M KOH solution at…

A: Volume of HCNO = 80.0 mL Molarity of HCNO = 0.4857 M Volume of KOH = 0.8029 M pkaof cyanic acid =…

Q: Methylamine Ethylamine H3NH₂ C₂H5NH₂ H₂NH3 C₂H5NH3+ 4.38 X 10 5.6 x 10-4 Aniline CH;NH, C6H5NH3 +…

A:

Q: Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer…

A: We have find out the values of PKb by using formula PKb= -log kb.

Q: What is the pH of the solution formed when 1.13 g of diethylammonium chloride ((CH3CH2)2NH2)+Cl- is…

A: Buffer solution: A buffer solutions is an aqueous solution consisting of a mixture of a weak base…

Q: Which of the following is true of a buffer solution that contains equivalent amounts of acid and…

A: buffer solution that contains equivalent amounts of acid and conjugate base means [Conjugate base ]…

Q: Part B Consider the following reaction: H2 (9) + I2 (g) = 2 HI (g) A reaction mixture at equilibrium…

A:

Q: lytical chemist is titrating 161.4 mL of a 0.8000M solution of trimethylamine ((CH3),N) with a…

A: HIO3 is an strong acid,  left amount of HIO3 deside the PH  of solution

Q: DH of the base solution after the chemist has added 484.1 mL of the HNO, solution to it. db nced…

A: Given,  Molarity of base =0.270 M Volume of Base = 234.9 mL Mmol of Base =  M × V   = 234.9 × 0.27 =…

Q: An analytical chemist is titrating 123.0 mL of a 0.5600M solution of diethylamine ((C₂H₂)₂NH) with a…

A: we have to calculate the pH of the solution

Q: formic acid buffer is prepared with 0.010 M each of formic acid (HCOOH) and Sodium formate (NaCOOH).…

A:

Q: Suppose a biochemist has 10 mL of a 1.0 M solution of a compound with two ionizable groups at a pH…

A:

Q: Histidine has ionizable groups with pKa values of 1.8, 6.0, and 9.2, as shown below (His = imidazole…

A: The three pKa values shows that there are 3 replaceable hydrogens in the molecule(represented as…

Q: A student wishes to make a buffer that has a pH of 4.65.  The student has HNO2 and NaNO2.  Nitrous…

A: A buffer solution is the mixture of weak acid and its conjugate base. It is also formed by the…

Q: A 0.030 M solution was prepared by dissolving potassium valinate in 1 L of water. What is the pH of…

A: pH is defined as the negative logarithm of hydrogen ion concentration present in the solution. pH =…

Q: One of the buffer systems the human body has to regulate pH is based on the phosphate anion. If…

A: A buffer works best at the pH near to the pKa value of the involved acid. First calculate the pKa…

Q: (CH3)2O →BF3(g)⇋BF3(g)+(CH3)2O(g) If you place 1.2 g of the complex in a 61.5 mL flask at 125 ℃,…

A: Answer: In the chemical equation complex is getting decomposed into two new compounds an equilibrium…

Q: Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer…

A: Given: Concentration of salt = 0.48 M pH = 9.75 Kb of methylamine = 4.38×10-4

Q: ) Determine the mass (in grams) of sodium formate that must be added to 1.00 L of 0.180 M formic…

A:

Q: A solution is prepared by adding 41 mg of sodium acetate (CH3COONA) to 1 L of distilled water. The…

A: The concentration of CH3COO- is needed to be determined in a solution prepared by dissolving 41 mg…

Applications of Molecular Spectroscopy

When light sources pass through the diffraction grating then light splits into different wavelengths. The light source produces two types of patterns that are shown as destructive and non-destructive. The light source is in the form of quanta that is quantitation.