A. What is the pH of a 350 mL buffer containing 0.125 mol HCOOH and 0.150 mol HCOONa? Ka=1.70x10-4 B. Propionic acid, CH3CH2COOH, has a Ka of 1.3x10-5 M. What mass of CH3CH2COONa would have to be added to 1.00L of 0.500M propionic acid for a resulting solution of pH=5.00?

Q: A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kb (C2H5NH2) =…

A: Given: 0.175 moles C2H5NH3NO3 0.225 moles C2H5NH2 V = 800.0 mL Kb (C2H5NH2) = 4.3 x 10-4

Q: A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kb (C2H5NH2) =…

A: pH of a buffer solution is calculated from Henderson Equation. If HCl is added to a buffer system pH…

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka=1.75X10°). Calculate the…

A: Given,  Molarity of CH3COOH = 0.40 M  Volume of buffer = 200.0 mL = 0.200 L Molarity of CH3COONa =…

Q: A 500.0 mL buffer solution is 0.150 M in acetic acid (Ka = 1.8 x 10–5) and 0.350 M in sodium…

A:

Q: emistry A 110.0-mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br. The Kb value for NH3 is…

A: The answer is as follows:

Q: How many grams of solid sodium cyanide should be added to 1.00 L of 0.116 M hydrocyanic acid…

A: Given-> Volume of HCN = 1.00 L Molarity of HCN = 0.116 M pH = 9.990  Ka(HCN) = 4.00 × 10-10

Q: EXTRA. What mass (g) of potassium fluoride (MW = 58.10 g/mol) must be added to 450. mL of a 0.100 M…

A:

Q: Consider the bases in the table. Which base would be the best choice for preparing a pH =…

A: Henderson-Hasselbalch equation: This equation is used to calculate the pH values for the buffer. For…

Q: How many grams of KHCOO (MM = 84.12 g/mol) must be added to 1.00 L of 0.256 M HCOOH to make a buffer…

A: pH of an acidic buffer solution can be calculated from Henderson hasselbalch equation. pH = pKa +…

Q: What quantity in moles of CH3NH3CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH₂ (Kb…

A: To calculate the number of moles of salt needed to prepare a buffer of given pH

Q: How many grams of solid potassium fluoride should be added to 1.00 L of a 0.140 M hydrofluoric acid…

A: Given -Volume= 1.00L Concentration of hydrofluoric acid= 0.140 M pH= 4.097 Ka(HF)=7.20×10-4Mass of…

Q: Determine the mass of NaF that needs to be added to 500.0 ml 0.100 M HF to produce a buffer with a…

A: Henderson's equation in terms of moles- pH=pKa+ logmoles of conjugate basemoles of weak acid

Q: Calculate the mass of C5H5NHCI (molar mass = 113.56 g/mol) that must be added to 0.80 L of 2.5 M…

A: Given, Kb of C5H5N( weak base)  is 1.8 X 10-9Therefore, pKb = - log(Kb)                            =…

Q: How many moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: A 175 mL buffer solution is 0.177 M in HONH2 and 0.149 M in HONH3 CL What is the pH of the solution…

A:

Q: Part A A beaker with 1.30×102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a…

A: We are given a beaker with 130 mL of an acetic acid buffer with a pH of 5.000 is sitting on a…

Q: A solution containing .30 M methylamine (CH3NH2) and .33 M methylamonium chloride (CH3NH3Cl) has a…

A: 1. Given that,  Concentration of CH3NH2 = 0.33 M Concentration of CH3NH3Cl = 0.30 M pH of the mixed…

Q: A buffer is made by dissolving 12.4 g of sodium dihydrogen phosphate, NaH,P04, and 21.8 g of…

A: pH means the negative logarithm of hydronium ions. By using Henderson - Hasselblach equation: A is…

Q: 1.0 L of a buffer solution was made with 0.15M in HOCl (Ka = 3.5 × 10-8) and 0.25M NaOCl. If 10.0 mL…

A: Number of moles of HOCl = 0.15 M * 1.0 L = 0.15 mol Number of moles of ClO–= 0.25 M * 1.0 L = 0.25…

Q: What is the pH of a buffer produced by mixing 250 mL of 0.521 M NH3 with 350 mL of 0.123 M NH4Cl ?…

A: We have to calculate the pH of the buffer solution

Q: Why is [H3O] = [OH-] + 1.0 X 10-2 M not feasible in water? What would happen if we tried to make…

A: Since you have posted 2 unrelated questions, hence they are considered as separate questions. And we…

Q: Phosphoric acid is a triprotic acid (K, = 6.9 x 10- M, K2 = 6.2 x 10-* M, and K = 4.8 x 10-1 M). To…

A:

Q: Find the pH of a buffer that consists of 0.34 M NH, and 0.17 M NH Cl. Round your answer to 2 decimal…

A: Data given:The concentration of ammonia, NH3 = 0.34 MThe concentration of ammonium chloride, NH4Cl,…

Q: The K₂ for the acid HX is 2.714. 10-5. How many moles of Nax need to be mixed with 2.586 L of 0.152…

A: We will first determine the moles of acid. we  know pKa= -logka,we will make use of equation-

Q: A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kb (C2H5NH2) =…

A: The pOH of a basic buffer solution can be expressed as: pOH = pKb  + logC2H5NH3NO3C2H5NH2pOH = pKb…

Q: Calculate the [H3O+] of 114.48 mL of a buffer initially consisting of 0.1320 M NH2OH and 0.1429 M…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: Salt of strong acid and strong base are neutral  Salt of strong acid and weak base is acedic and…

Q: c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results are…

A: Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated…

Q: A 1.000L buffer is made of 0.7 M CH3COOH and 0.6 M CH3COONa.What is the pH of the buffer solution?…

A: The pH of the buffer solution can be determined as follows: pH = pKa + logSaltAcidpH = 4.74 +…

Q: A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kb (C2H5NH2) =…

A: The pH of the given buffer solution of C2H5NH3NO3 and C2H5NH2 is;…

Q: A buffer composed of 0.1 M CH3COOH/1.0 M CH3COO- has a lower buffering capacity as opposed to a…

A: We know that, buffer capacity range from ( pKa + 1 ) to ( pKa - 1 )  Buffer capacity very less at…

Q: A buffer is prepared by mixing 16 mL 1M CH3COONa and 4 mL 1M CH3COOH pKa = 4.74. Determine the pH…

A: Initial no. of millimoles of CH3COONa = ( 16 × 1) = 16 millimoles Initial no. of millimoles of…

Q: A buffer solution made with HCN and NACN has a pH of 9.16. Which statement is true? Ka(HCN) =…

A:

Q: i. A 1.000L buffer is made of 0.7 M CH3COOH and 0.6 M CH3COONa .What is the pH of the buffer…

A: (i) We have  volume of solution =1 L Molarity of CH3COOH=0.7 M⇒moles =0.7 mol/L ×1L=0.7 molMolarity…

Q: A lactic acid/lactate ion buffer solution contains 0.45 M HC3H; O3 and 0.79 M C3H5O3 , respectively.…

A: Given values -> [HC3H5O3]=0.45M [C3H5O3^-]=0.79M Ka = 1.4 × 10^-4

Q: You make a buffer using 250mL of 0.500M sodium acetate and 250mL of 0.500M acetic acid. How many mL…

A: A buffer solution is a solution that resists the change of pH upon the addition of a small amount of…

Q: What quantity in moles of HCI need to be added to 200.0 mL of a 0.200 M solution of NaF to make a…

A: moles of HCl added to prepare the buffer solution

Q: Suppose there is 1.00 L of an aqueous butfer containing 60.0 mmol of acetic acid (pk, = 4.76) and…

A: Given,  Moles of weak acid, CH3COOH = [CH3COOH] = 60.0 mmol  Moles of salt, CH3COONa = [CH3COONa] =…

Q: 1.00L of  a buffer is created to be 0.100M in HOAc and 0.100M in NaOAc. What is the pH of the…

A:

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka= 1.75X10-5). Calculate the…

A: Mn

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.