A buffer solution is made using a weak acid, HA , that has a pK of 5. If the pH of the buffer is 6, what is the ratio of [A-] to[HA] ?(A"][HA]4.05 x1023+ Post a new auestionétv A A4MacBook Pro$&46.78.9.RYUP%3DFGHJK....ト

Given :- pKa for weak acid HA = 5 pH of buffer solution = 6 To calculate :- ratio of…

Answered: A buffer solution is made using a weak…

A buffer solution is made using a weak acid, HA, that has a pk, of 5. If the pH of the buffer is 6, what is the ratio of [A-] to [HA]?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 121CP: A buffer is made using 45.0 mL of 0.750 M HC3H5O2 (Ka = 1.3 105) and 55.0 mL of 0.700 M NaC3H5O2....

See similar textbooks

Related questions

Q: What are the speculator ions in 2HCl(aq)+ BaSO4(s)-> BaCl2(aq) + H2SO4(aq)

Q: What are the products of the following decomposition? Ni(CIO3)2 -->

Q: The concentration of SrCO3 in a saturated aqueous solution of salt at 25°C is 3.05 x 10 M. What is…

A: Given Chemical Reaction SrCO3 ( S ) ------------> Sr+2 ( aq ) + CO3 2- ( aq ) Solids and…

Q: What is the pH of a 50 cm3 buffer solution if it is contains 0.0100 mol/dm3 sodium acetate and…

A: Acids are categorized as strong acids and weak acids based on the degree of dissociation it…

Q: A buffer system is set up with [HA] = 2[A–]. If pKa = 5.5, what is the pH of the buffer?

Q: Use pka values to predict which of the following equilibria will favor the reactants.

Q: What is the pK of the weak acid HA if a solution containing 0.1 M HA and 0.2 M A− has a pH of 6.5?

Q: Alizarin yellow R, Ka=7.9×10−12, is yellow in its protonated form (HX) and red in its ionized form…

A: Given, Ka = 7.9*10-12. It is yellow in color in protonated form (HX) and red in color in ionized…

Q: A buffer solution is made using a weak acid, HA, that has a pK, of 4. If the pH of the buffer is 1,…

Q: Chemistry How do I calculate the %ionisation at pH of a drug (compound code;UQPC 22-606-Q) the “Q”…

A: percent ionization = [H+]/[unionized form ] ×100

Q: a. What is the pH of a 0.20 M solution of sodium acetate? The Ka for acetic acid is 1.8 x 10⁻⁵? b.…

A: We have to calculate the pH of the given solution. a. Given that, the concentration of sodium…

Q: How can the electrons in a catalyst (complex) be counted in neutral and in ionic form? When do the…

A: There are two methods for counting electrons.Neutral or covalent method or effective atomic no or…

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.100 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 ×…

A: Concentration of CH3NH2 = 0.400 M Concentration of CH3NH3I = 0.100 M Kb for CH3NH2 = 4.4 × 10-4 pH…

Q: 18. Calculate the pH of the solution formed when 12.0g of sodium fluoride (0.286mol) (NaF, FW- 41.99…

A: For a buffer- pH = pKa + log[Base][Acid] Now, pKa = - log Ka = 3.19 [Acid] = 0.5 M [Base] = 0.286…

Q: Please draw the structures of the products (equimolar mixtures of reactants) for the following…

A: In inorganic chemistry, the trans effect is the labilization of ligands that are trans to certain…

Q: The o-complex formed for the bromination of benzoic acid should be Br, H COOH COOH COOH Br (a) (b) +…

A: Since, you have asked multiple questions. We will solve the first question for you. To get the…

Q: What is the pH of a solution containing 0.327 mol L-1 of HCl and 1.041 mol L-1 of a weak acid with…

Q: Fe3+ (aq) + SCN¯(aq)= FENCS²+*(aq)

A: The principle used to maintain the balance between both sides of the reaction is Le Chatelier's…

Q: The pH of the buffer solution that formed between CH3COOH and CH3COONa is 4.97. What is the ratio of…

A: pH is used to determine the concentration of hydronium ion.

Q: What is the pH of a boric acid buffer solution containing 0.18 mol/L of boric acid, НзВОз, and 0.12…

A: Introduction : We have to calculate pH of boric acid .

Q: What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9?…

Q: A hypothetical weak acid, HA, was combined with NaOH in the following proportions: 0,20 mol HA, 0,08…

Q: HCECH + но HCEC + H,0 b) OH H + Но H + H,0

Q: calculate the equilibrium concentration of FeSCN2+

A: Equilibrium is the state of the reactions in which the reactant converts product and product convert…

Q: Consider a buffer solution that is 0.50 M in NH and 0.20 M in NH4Cl. For ammonia, pKp = 4.75.…

Q: 6. The pKa of lactic acid (CH3CH(OH)COOH) at 298 K is 3.85 write the equilibrium expression for this…

A: Lactic acid is a weak acid. The weak acid dissociates partially in the aqueous solution to give…

Q: 1-For the reaction, 4 Cl- + Co(H2O)62+ CoCl42- + 6 H2O (color 1)…

Q: A buffer solution is made using a weak acid, HA . If the pH of the buffer is 7 and the ratio of [A−]…

Q: range of pH values could be achieved with a buffer consisting of nitrous acid and sodium nitrite?…

A: Nitrous acid is a weak acid and sodium nitrite is its salt. So, here we have to use the Henderson…

Q: Calculate the masses of Ni(OH)2 that will dissolve in the following solvents Ksp Ni(OH)2 = 6.0x10-16…

A: Part A Let the solubility of Ni (OH)2 in 250 mL of water be ‘s’ Ksp = [S][2S]2 Ksp = 4S3 6 x 10-16…

Q: Calculate the molar concentration of a purified enzyme (MW 25000 Dal) in a solution of 0.10 g/ml of…

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

Q: Calculate the pH of a 0.20 M HA solution, given the pKa of HA is 2.22.

Q: NOH2PO4 and Na2HPO4 For what ratio between the concentrations of the two substances above would the…

A: The given buffer solution is a mixture of weak acid NaH2PO4 and conjugate base Na2HPO4 . The pH of…

Q: The p Kp of ethylamine is An analytical chemist is titrating 195.8 mL of a 0.6200 M solution of…

A: Given that: Volume of of ethylamine (C2H5NH2) solution = 195.8 mL = 0.1958 L, Molarity = 0.6200 M…

Q: The hydronium ion concentration in a solution of an unknown weak acid is 5.77 x 1011. What is the…

A: Pka value is depends upon concentration of H+ ions in the solution.

Q: The Ksp of CaF2 is 1.5 x 10-10. If CaF2 (s) is dissolved in pure water, what is the solubility in…

A: We have to calculate the solubility of CaF2 in water .

Q: Acetic acid was dissolved in water to a concentration of 0.10 mol.L-. The pKa of acetic acid is 4.8.…

A: a.) Acetic acid is an acid , so it would donate protons . For this we would write a chemical…

Q: Fluoride treatment strengthens tooth enamel by converting hydroxyapatite, Cas(PO4)3OH, into…

A: Solubility product (Ksp) basically exhibits equilibrium that exists between particular solid and its…

Q: One of the following indicators or species or mixtures is colorless in acidic solution? a. Starch-l3…

A: In this question, we will see which can not give color in acidic solution means it should be remain…

Q: Identifying Reaction Types Identify the reaction type shown and describe the clues that were used to…

A: Chemical reactions can be classified into different types , such as Decomposition reactions…

Q: Carbonic acid, H2CO3, undergoes the following acid base equilibria: H2CO3,=H*(aq) + HCO;¯(aq) =…

A: The relation between pKa and pH can be known as, ph = pKa + logsaltacid

Q: Calculate the pH of a 0.100 M alanine (HL/intermediate form) solution. pKb1 = 4.29 and pKb2 =11.67.

Q: What is the Ksp for the following reaction if the concentration of La3+ was measured to be 9.2 ×…

Q: What is the pH of a buffer solution that contains 0.245 M weak acid and 0.450 M of the conjugate…

Q: A3B5 and a Ksp of 7.6E-26.

A: The pB value for given conditions is 3.75

Q: What is the reducing agent in the following reaction?2 Br-1aq2 + H2O21aq2 + 2 H+1aq2 ¡ Br21aq2 + 2…

A: The species which lose electrons undergo oxidation. The species which accepts electrons undergo…

Q: Which of the following could be added to a solution of monobasic dihydrogen phosphate (KH2PO4) to…

A: A buffer solution is that which resist change in pH when acid/base is added in small amount.

Q: what is the pKa of the acid?

A: Given :- pH of solution = 4.9 Concentration of conjugate base = x Concentration of acid = 2.3 x…

Question

A buffer solution is made using a weak acid, HA , that has a pK of 5. If the pH of the buffer is 6, what is the ratio of [A-] to
[HA] ?
(A"]
[HA]
4.05 x1023
+ Post a new auestion
étv A A
4
MacBook Pro
$
&
4
6.
7
8.
9.
R
Y
U
P
%3D
F
G
H
J
K
....
ト

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Equilibrium Concepts in Analytical Chemistry

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). List the major species, and explain how you would go about calculating the pH of the solution at various points, including the halfway point and the equivalence point.
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
A buffer is made using 45.0 mL of 0.750 M HC3H5O2 (Ka = 1.3 105) and 55.0 mL of 0.700 M NaC3H5O2. What volume of 0.10 M NaOH must be added to change the pH of the original buffer solution by 2.5%?
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
The desired pH is 6.4 in creating a buffer system/buffer solution of about 50-60mL. Therefore, a student picks Silicic Acid Si(OH)4, as 1mL of 1M of the acid has a pH of 6.4, which also has a pKa of 9.82. What is the ratio HA/A- and ratio A-/HA-? The buffering capacity will be checked by the addition of 1mL of 1M HCl or 1mL of 1M NaOH and should not change by more than 0.25pH units.
A buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?
A buffer system has 3[HA]=[A-]. Given that the pKa is 7.2, what is the pH of the buffer solution at 25°C? Please space stuff out, everything has been written together as a single line so it is difficult for me to figure out what was written
What is the resulting pH when 0.005 moles of KOH is added to 0.100L of a buffer solution that is 0.100 M in H2PO4- and 0.100 M HPO42- and the Ka2=6.2x10-8?
Suppose 100 mL of 2.0 × 10–4 M Fe(NO3)3is added to 100 mL of 2.0 ×10–5 M KIO3. What is Qsp value? Will it precipitate?
A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3HO-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 200.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.)
What is the molar solubility of a hypothetical compound AB in a solution containing 19.92 M B- given a Ksp = 1.706 x 10-2? AB(s) ⇌ A+(aq) + B-(aq) 8.56e-4 6.56e-3 3.82e-3 2.93e-2
What is the pH of a 1.0 L solution that is 0.50 M PO43- and 0.50 M HPO42-? (The pKa values for H3PO4are: 2.14, 7.2, and 12.4 respectively) If 0.01 moles of OH- is added to the above buffer, what will the new pH be? Change of volume is negligible. If 0.01 moles of OH- is added to 1.0 L of water, what will the new pH be? Change of volume is negligible.