Answered: If a buffer solution is 0.260 M in a…

If a buffer solution is 0.260 M in a weak base (Kp = 1.4 x 10-5) and 0.560 M in its conjugate acid, what is the pH? pH =

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter8: Acids And Bases

Section: Chapter Questions

Problem 8.60P: 8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?

See similar textbooks

Related questions

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: We know that, pH can be expressed as negative logarithm of H+. i.e., pH = -…

Q: What is the pH of the buffer solution that contains 1.6 g of NH4Cl in 250 mL of 0.060 M NH3? Is the…

A: pH of a basic buffer can be calculated using Henderson-Hasselbach equation: pH=14-(pKb+logB+BOH)

Q: Calculate the K of a weak monoprotic acid if a 0.10 M aqueous solution of the acid has a [H*] of…

A: Given, Concentration of the monoprotic acid solution (C) = 0.10 M Concentration of the Hydrogen ion…

Q: If Kal for H2 CO3 is 4.20 x 10-, what is the pH of the buffer solution? pH = Write the net ionic…

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: A buffer solution is made that is 0.397 M in HCN and 0.397 M in KCN. If K, for HCN is 4.00 x 10-10,…

A: Acidic buffer pH = pKa + log[salt]/[acid] pKa = - logKa = - log4 x 10-10 = 10- log…

Q: What is the pH of a buffer made from 0.580 mol of CH₃NH₂ (Kb = 4.4 × 10⁻⁴) and 0.180 mol of CH₃NH₃I?

A: Concentration of CH3NH2 = 0.580 Concentration of CH₃NH₃I = 0.189 Kb = 4.4 × 10-4 pH = ?

Q: Consider the reaction of a 20.0 mL of 0.220 M C̟H̟NHCI (Ka = 5.9 x 10*) with 12.0 mL of 0.241 M…

A: Given molarity of C5H5NHCl or C5H5NH+ = 0.220 M Volume of C5H5NHCl solution = 20.0 mL = 0.020 L…

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: A buffer solution is made that is 0.355 M in HCN and 0.355 M in KCN. If K, for HCN is 4.00 x 10-10,…

A: We have to find the pH of the given buffer solution

Q: A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the…

Q: If the system CaCO3(s) + 2H+(aq) --> Ca2+(aq) + CO2(g) + H2O(l) is saturated with respect to CaCO3,…

A: In the system, CaCO3(s) + 2H+(aq) --> Ca2+(aq) + CO2(g) + H2O(l) we can see that H+ is reacting…

Q: A buffer solution is 0.200 M in HC,H;O2, a monoprotic acid, and 0.200 M in NaCH,O2. K, for the acid…

Q: What is the pH of a boric acid buffer solution containing 0.25 mol/L of boric acid, H3BO3, and 0.50…

Q: A weak base has a base hydrolysis constant, Kp, of 5.5 x 10-6. What is the pH of a 0.21 M solution…

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the given…

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: Q-4- calculate the molar solubility of Barium iodate 1- in distilled water 2- in Barium nitrate…

Q: The solubility product constants of PbSO4 and SrSO4 are6.3 x 10-7 and 3.2 x 10-7, respectively. What…

A: Solubility product is equilibrium constant of a reaction where an ionic compound in solid form…

Q: What is the pH of a buffer that is 0.41 M HCN(aq) and 0.87 M NaCN(aq)? The Ka of HCN is 6.2 x 10-10.

A: Using Henderson Hasselbalch equation we can calculate pH of a buffer

Q: A buffer solution is made that is 0.378 M in H2 CO3 and 0.378 M in KHCO3. If Ka1 for H2 CO3 is 4.20…

A: PH of a buffer solution given by Henderson's equation as follows PH=PKa +…

Q: A buffer is prepared containing 0.1 M of a weak acid HA (Ka=1x10-8) and 0.2 M of its conjugate base…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: A solution is prepared by dissolving 1.800 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.180…

Q: The ammonia ion NH4+ has a Kz of 5.6 x 10-10. What is the K, for the base ammonia? Kp

A: Ka is the . ionisation constant for acid and kB is for base. Use relation between them and get the…

Q: A buffer solution is 0.374 M in H2 S and 0.205 M in KHS. If Ka1 for H2S is 1.0 x 10-7, what is the…

A: when a weak base and its salt are present in solution, they form a buffer solution.

Q: What is the pH of a 0.24 M solution of oxalic acid, H2C204? The K31,2 values of oxalic acid are 5.6…

Q: At 22 ∘C, an excess amount of a generic metal hydroxide, M(OH, is mixed with pure water. The…

Q: Calculate the pH of a buffer solution that is 0.450 M HA and 0.550 M A-. Ka = 1.30 x 10-4

A: The pH of any Buffer System can be calculated by following the simple equation known as Handerson…

Q: What is the pH of a 0.681 M weak base solution? The Kp of the weak base is 0.000098.

A: Given:: Let HB is weak base then, [HB] =0.681 M Kb=0.000098

Q: 10.0 ml of HCl was added to 100.0 ml of a 0.2 M solution of NH4Cl (Ka=1.8x10-5). If the resulting…

A: Given: 10.0 ml of HCl was added to 100.0 ml of a 0.2 M solution of NH4Cl (Ka=1.8x10-5). If the…

Q: Mix 10.0 cm3 of 0.2 M sodium-acetate solution and 10.0 cm3 of 0.3 M acetic acid solution. What is…

A: Value of pH is sued to calculate acidity or basicity of a solution. At room temperature, pH value…

Q: What will be the pH of a buffer

A: Given :- Concentration of weak acid i.e. HCN = 0.65 M Concentration of conjugate base i.e. CN- =…

Q: What is the pH of a buffer made from 0.580 mol of CH₃NH₂ (Kb = 4.4 × 10⁻⁴) and 0.120 mol of CH₃NH₃I?

A: In this question, we want to determine the Calculate the pH of the buffer solution. You can see…

Q: What is the pH of a buffer composed of 0.35 M H2PO4–(aq) and 0.65 M HPO42–(aq)? (Ka of H2PO4– is 6.2…

A: Ka of H2PO4– = 6.2 x10–8 pKa of H2PO4– = - log Ka = - log 6.2 x10–8 = 7.2

Q: A weak base, B, has a Kp value of 5.3 x 10-4. What is the hydroxide ion concentration in a 0.050 M…

A: Given-> Kb = 5.3 × 10^-4 Concentration = 0.050 M

Q: Which acid, along with it's corresponding salt, would be best to make a buffer of pH 7? hydrofluoric…

A: Given pKa = -log KaHydrofluoric Acid = Ka = 6.8 × 10-4pKa = 3.2Hypochlorous Acid = Ka = 3.5 ×…

Q: A weak acid is added to a strong base. The base is neutralized last, giving a mole ratio to acid…

Q: The solubility of salts that contain the conjugates of weak acids increase in acidic solution. Given…

A: The solubility product of CuCN is given as:CuCN (s) ⇌ Cu+ (aq) + CN- (aq)Solubity product, Ksp =…

Q: Consider the following buffer system: 1.03 M H3PO4 and 0.93 M H₂PO4-. What is the pH of such a…

A: Acidic buffer :- A mixture of weak acid and its salt with strong base is known as acidic buffer…

Q: The solubility constant of lead (II) hydroxide [Pb(OH)2] is 1.2 x 10-15. If 100.0 g of this…

A: The molar solubility (s) of [Pb(OH)2] is calculated as shown below. On substitution, the molar…

Q: What is the pH of 0.33 M acetic acid to 1.00 L of which 1.44 g of sodium acetate, NaCH3 CO2, has…

A: Given: The molarity of acetic acid = 0.33 M The mass of sodium acetate added = 1.44 g The volume of…

Q: You are titrating 21.00ml of a 0.850 M solution of NH3(ammonia) with a strong acid. If you add…

A: A basic buffer is acquired on mixing weak bases with their conjugate salts in a definite ratio. They…

Q: If the Kp of a weak base is 7.3 x 10-6, what is the pH of a 0.28 M solution of this base? pH =

A: The value of Kb for the given weak base is = 7.3x10-6 The concentration of the base solution is =…

Q: A buffer solution is 0.402 M in H2CO3 and 0.314 M in KHCO3. If Kal for H2CO3 is 4.2 X 10 -7 , what…

Q: 0.020 mol of solid NaOH to 1.0 L of the solution?

A: Moles of CH3COOH = M × V(L) = 0.50 × 1.0 = 0.50 mol Moles of CH3COONa = 0.50 × 1.0 = 0.50…

Q: A certain weak base has a Kp of 8.20 × 10–7. What concentration of this base will produce a pH of…

A: We have to calculate the concentration of the base.

Q: A buffer solution is 0.351 M in HCN and 0.733 M in NaCN. If K, for HCN is 7.5 x 10-10 at a certain…

A: Given Concentration of HCN = 0.351 M Concentration of NaCN = 0.733 M Ka for HCN = 7.5*10-10

Q: If the Kp of a weak base is 1.8 x 10-6, what is the pH of a 0.24 M solution of this base? pH =

A: Below attached file showing the details answer. All the best.

Q: Lactic acid has a K. of 2.502 x 103. A solution contains 0.275 M lactic acid and 0.375 M sodium…

A: Buffer solution: The mixture of lactic acid and sodium lactate act as a buffer solution. The…

Q: 1) Write the equilibrium constant expression for the following reaction. CaO(S) + 2HCl (aq) CaCl2…

A: Answer 1 :- We have to find out the equilibrium constant for the following given reaction., CaO(S) +…

Question

100%

If a buffer solution is 0.260 M in a weak base (Kp = 1.4 x 10-5) and 0.560 M in its conjugate acid, what is the pH?
pH =

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

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

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 pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7 ?
What is the pH at 25degrees Celsius of a saturated solution of silver hydroxide? (Ksp value for silver hydroxide is 2.0 x 10^-8)
A buffer solution is 0.402 M in H2CO3 and 0.314 M in KHCO3. If Kal for H2CO3 is 4.2 X 10 -7 , what is the pH of this buffer solution? pH =
A solution saturated in calcium hydroxide Ca(OH)2,has a PH of 12.35. Calculate the Ksp for calcium hydroxide
Calculate the pH of a buffer solution that is 0.100 M acetic acid and 0.200 M sodium acetate.The Ka of acetic acid is 1.8 x 10-5.
What of the following is the expression for the solubility product of Ba3(AsO4)2?
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction?
At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.16. What is the Ksp of the salt at 22 °C?
You are titrating 21.00ml of a 0.850 M solution of NH3(ammonia) with a strong acid. If you add 1.20ml of a solution of a 1.80M solution of hydrochloric acid, what is the final pH of the resulting solution? The Kb for ammonia 1.77x10^-5
For a solution that is 0.50 M in NH3 (Kb =1.8 x 10-5) and 0.25 M in NH4Cl, find pH and pOH
We titrate a solution containing 10 mL of CH3COOH 0.1095 mol/L and 90 mL of distilled water, with NaOH 0.09220 mol/L, a strong base. What is, at equilibrium, the concentrations of H3O+, CH3COO-, CH3COOH and the initial pH (of the acid) before starting the titration?