14. Acetic acid has a Ka of 1.8 x 10-5. What is the pH of a buffer solution containing 0.15M HC2H3O2 and 0.15M C2H3O2?

Q: The pH of a 500.00 mL buffer solution containing sodium mandelate and mandelic acid (ka= 3.89×10-4)…

A: Given, Volume of buffer solution (V) = 500 mL  Ka = 3.89 x 10-4  αo = 0.90  To find : pH

Q: 3.2. Calculate the mass of NH&CI that should be dissolved in 525.00 mL of 0.1531 M NH3 (Ko = 1.8 x…

A:

Q: Consider a 25.0 mL buffer solution containing 0.100 M sodium alderate and 0.126 M alderic acid. What…

A:

Q: A buffer is prepared containing 0.250 M NH3 and 0.253 M NH4Cl. Calculate the pH of the buffer. The…

A: Use the formula of buffer solution to calculate pH for buffer solution and calculate Ka value using…

Q: What is the pH of a buffer that is 0.120 M in formic acid (HCHO2) and 0.080 M in potassium formate…

A: Given, Ka = 1.8 * 10-4. a) 2.33 b) 3.57 c) 3.74 d) 3.91

Q: What is the pH of a buffer that is0-08 M NaA and D.1 HA The ka of AA =1-0 x 104 a 2.16 b. 3.91…

A: In multiple questions, we solve only one question according to Bartleby guidelines. If you want…

Q: HCN] ka=4.0x10^-10    pka=10.32 An aqueous solution contains 0.447 M hydrocyanic acid. How many mL…

A:

Q: Calculate the pH of a buffer of a mixture of 0.450 M propionate and 0.342 M propionic acid.…

A: Henderson equation,pH of the buffer solution is calculated by using Henderson equation, it is,

Q: A 75.0 mL sample of 0.05 M HCN (pKa = 9.21) is titrated with 0.5 M NAOH. What is [H3O*] in the…

A:

Q: What is the pH of a buffer solution that is 0.30 M chloroacetic acid and 0.17 M sodium…

A: Since chloroacetic acid is a monoprotic acid.

Q: What is the pH of a buffer made by

A: acidic buffer pH is  pH = pKa + log[salt]/[acid]   ------(1) pKa = - logKa = - log 1.82 x 10-4…

Q: Calculate the molar solubility of Ni(OH)2 (Ksp = 6x10-16) in !3! (1) pure water (2) pH = 2.00 buffer…

A: #1. Pure water: The equation for the dissociation of Ni(OH)2 is: Ni(OH)2(s) ⇌ Ni2+(aq) + 2OH-(aq)

Q: 15.0 mL of 0.475M CH3COOH is titrated with 0.450 M RbOH. What is the pH after 18.0 mL of RbOH has…

A: Given: Concentration of CH3COOH= 0.475M Volume of CH3COOH=  15.0mL Concentration of RbOH = 0.450M…

Q: 8. What is the pH of a buffer solution made with 0.53M benzoic acid with Ka = 6.5 x 105 and 0.478M…

A:

Q: A solution contains 0.250 M HA (Ka = 1.0 x 10-6) and 0.45 M NaA. What is the pH after 0.30 mole of…

A: The pH is calculated below.

Q: To prepare a buffer solution containing CH 3 CO 2 H and NaCH 3 CO 2 , and having a pH of 5,what…

A: A buffer solution is a solution which resists any change in it's pH value on addition of small…

Q: Calculate the pH of a buffer solution made of 0.35 M H2CO3 and 0.20 M NaHCO3. Ka=4.3x 10^-7 for…

A: pH is defined as negative logarithmic of concentration of hydronium ion

Q: What is the pH of the buffer that is composed of 0.10 M Na2HPO4 and 0.15 M KH2PO4? (Ka1=7.5 x 10~³,…

A: Given: Concentration of Na2HPO4 i.e. conjugate base of KH2PO4 = 0.10 M And the concentration of…

Q: You have 500.0 mL of a buffer solution containing 0.30 Macetic acid (CH₂COOH) and 0.20 M sodium…

A: Volume of buffer solution = 500 mL = 500 × 10-3  L Molarity of  Acetic acid = 0.30 M Molarity of…

Q: What olume of 17.1 M glacial acetic acid (HC2H3O2) must be added to 100.0 mL of 1.25 M KOH to form a…

A: Given, Molarity of glacial acetic acid=1.71M Volume of KOH=100mL Molarity of KOH=1.25M pH of…

Q: What is the pH of a buffer solution that is 0.159 M in hypochlorous acid (HCIO) and 0.121 M in…

A: Given: Concentration of hypochlorous acid (HCIO)=0.159 M Concentration of  sodium hypochlorite…

Q: How many grams of solid sodium acetate should be added to 1.00 L of a 0.275 M acetic acid solution…

A: A buffer solution is the one that resists any change in pH when acid or base is introduced in it in…

Q: 10.0 mL of 0.02 M carbonic acid (H2CO3) is titrated with 0.01 M NaOH. What is the pH of the carbonic…

A: The question is Based on the concept of titrations. we have to calculate carbonic acid solution pH…

Q: What is the pH of buffer solution containing 0.15 M acetic acid and 0.02 M sodium acetate? Lütfen…

A: Given 0.02 M acetate anion   0.15 Acetic Acid  pka oaf acetic acid = 4.75

Q: acid buffer containing 0.050 M CH3COOH and 0.050 M CH3COONA has a pH of 4.74. What will after 0.0020…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid .…

Q: What is the pH of a buffer solution that is 0.46 M chloroacetic acid and 0.29 M sodium…

A: Since chloroacetic acid is a monoprotic acid.

Q: A hypochlorous acid buffer is prepared with 0.10 moles HCIO and 0.10 moles CIO- and pH = pKa = 7.40.…

A: pH = pKa + log[salt]/[acid] ClO-  +  HCl  ----->  HClO  +   Cl- Number of moles of HClO formed =…

Q: Describe how to prepare 1.0L of 0.10M acetate buffer of pH=4.00, from given 0.10M solutions of…

A: The volume of acetic acid and acetate to be mixed is calculated as, pH = pKa + log ([A-]/[HA]) [A-]…

Q: A buffer solution containing only 0.050 mol of CH3NH2 and 0.060 mol of CH3NH3CI has a total volume…

A: When sodium hydroxide is added then hydroxide ion is react with salt and produced base of basic…

Q: What will be the appropriate pH of a buffer prepared by mixing 100 ml of 0.1 M Na2HPO4 and 100 ml of…

A: amount of given concentrations salt concentration Na2HPO4 = 100 ml X 0.1 M = 10 mmol acid…

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka= 1.75x10-5). Calculate the…

A:

Q: Which of the following would be the best choice for preparing a buffer with a pH = 8.0? Select one:…

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

Q: have to be added to 1.0 L of a 1.948 M HA solution in order to obtain a buffer of 3.11? (The Ka for…

A: We will use buffer equation

Q: A solution contains 0.250 M HA (Ka = 1.0 x 10-6) and 0.45 M NaA. What is the pH after 0.30 mole of…

A:

Q: The solubility of magnesium hydroxide in pure water is 1.3 x 10–4 mol/L. (a) Calculate the Ksp of…

A: (a) Dissociation reaction of Mg(OH)2 is given below,     Mg(OH)2  -------------> Mg2+ + 2OH- i…

Q: 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.250 M in NaC7H5O2. Calculate the pH of the…

A: Given that : Molarity of acid (HC7H5O2) = 0.150 MMolarity of salt (NaC7H5O2) = 0.250 MVolume = 1.00…

Q: What is the pH of a buffer prepared with 1.5 M NaC11H5O4, and 3.3 M HC11H5O4? Ka = 9.0X10 -4.36 4.50…

A:

Q: Aditi titrated 80.00 mL of 0.50 M ethylamine, CH3NH2, with 0.40 M HC CH3NH₂ Kb = 4.4 x 10-4 What is…

A: Kb = 4.4×10-4 pKb = 3.36 Molarity of base =0.50 M Volume of base = 80 mL M × V  Mmol of base =M × V…

Q: 1. Calculate the [H+] and the pH of a buffer solution that is 0.10 M in CH3COOH (Ka = 1.8 x 10-5)…

A: The  concentration of H+ and the pH of a buffer solution are calculated in step two.

Q: 18.00 mL 0.321 M what is the pH value of the solution when titration of NH3 a) 10.00 mL and b)…

A: The question is based on the concept of volumetric analysis. It involves titration of weak base…

Q: 3. 1. A sample of 50.0 mL of 2.0 M HNO2 (pKa=3.398) is titrated with 1.0 M KOH. Determine the pH…

A:

Q: Calculate the molar solubility of Ag2CO3 (Ksp= 8.1 x 10-12) in a solution buffered to a pH of 6.00?…

A: It is given that the pH is 6.00. thus, pH = -log H+= 6.00 H+= 10-6.00=1.0×10-6 M

Q: The pH of a Buffer containing 1.OM CH3COOH and 0.1M CH3COONA (pka of * :CH3COOH =4.74) is 3.0 O 4.74…

A: The pH of buffer containing 1.0M CH3COOH and 1.0M CH3COONa calculated as follows

Q: What olume of 17.1 M glacial acetic acid (HC2H3O2) must be added to 100.0 mL of 1.25 M KOH to form a…

A: Since moles of KOH = concentration of KOH X volume of KOH solution in L = 1.25 X 100 / 1000 = 0.125…

Q: What is the pH of 3.00 L of a buffer made of (2.840x10^-1) M HBrO and (7.16x10^-1) M KBrO AFTER the…

A: The buffer are those solution which shows very little variation in pH upon addition of a base or an…

Q: a buffer is created with 0.450 CH3COOH and 0.380M CH3COO- calculate the pH CHANGE if 0.042 mol NaOH…

A:

Q: What is the pH when 10 mL of 0.144 M HC2H3O2 ( Ka= 1.80*10^-5) is titration with 55 mL of 0.183 N…

A: The Henderson-Hasselbalch equation is, pH=pKa+logConjugate baseWeak acid

Q: Calculate the pH of a buffer solution consisting of 0.12 M NH3 and 0.095 M NH4+. The Kb for NH3 =…

A: Concept Introduction: pH is the log concentration of protons and pOH is the log concentration of…

Q: Choose the buffer with the greatest buffering  capacity:     d. 0.25M formic acid/formate buffer at…

A: We are given three different types of buffer solution at different pH and concentrations and we have…