A buffer solution is prepared by dissolving 0.200 mol of NaH 2PO 4 and 0.100 mol of NaOH in enough water to make 1.00 L of solution. What is the2-pH of the H 2PO 4/HPO 4buffer if the K a2 = 6.2 x 10 8?7.517.717.216.91Click Save and Submit to save and submit. Click Save All Answers to save all answers.Save All AnswersMacBook AirDD000000F10FF6F7F8F9F3F4F5F2)C@$424.567.8.9-TY.UPnWGJKSHILLR%# 3m

Buffer solution is the solution which has tendency to maintain constant pH upon addition of small…

A buffer solution is prepared by dissolving 0.200 mol of NaH 2PO 4 and 0.100 mol of NaOH in enough water to make 1.00 L of solution. What is the pH of the H 2PO 4/HPO 42- buffer if the K a2 = 6.2 x 10 -8? 7.51 O7.71 7.21 6.91

A buffer solution is prepared by dissolving 0.200 mol of NaH 2PO 4 and 0.100 mol of NaOH in enough water to make 1.00 L of solution. What is the pH of the H 2PO 4/HPO 42- buffer if the K a2 = 6.2 x 10 -8? 7.51 O7.71 7.21 6.91

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 46E: An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 M...

See similar textbooks

Related questions

Q: Calculate the pH at the equivalence point when 2.5 x 10-3 mol of hypochlorous acid are dissolved in…

A: Neutralization or equivalence points are achieved during titrations of finding unknown…

Q: An analytical chemist is titrating 94.8 mL of a 0.4000M solution of nitrous acid (HNO,) with a…

A: Given : Volume of HNO2 solution = 94.8 mL = 0.0948 L (since 1 L…

Q: Calculate the pH of a buffer solution that contains 0.34M benzoic acid and 0.49 M potassium…

A: Using Henderson equation , we can solve this problem. Here benzoic acid is weak acid and potassium…

Q: A titration is performed in which 0.27 M KOH is added to a 100.0 mL sample of 0.18 M HI. What is the…

Q: Calculate the pH of a buffer solution prepared from 0.35 mol of K3PO4, 0.250 mole of KH2PO4, and…

A: The dissociation equation is as follows:

Q: Consider the buffer system of ammonia, NH3 and ammonium ion NH4+ (Ka= 5.6 x10^-10) a) what is the…

A: Value of pH of a solution is used to measure the acidity or basicity of a solution. At room…

Q: Phosphoric acid is a triprotic acid (Kal 6.9 x 10-3, K2 = 6.2 × 10-8, and Ka3 = 4.8 x 10-13). To…

Q: A buffer solution is prepared in which the concentration of NH3 is 0.20 M and the concentration of…

A: Given : buffer solution of weak acid NH4+ and its conjugate base NH3 concentration of NH3 = 0.20 M…

Q: Calculate the buffer capacity of a buffer solution prepared by mixing 0.215M sodium acetate and…

A: Given = Concentration of sodium acetate = 0.215M Conc of acetic acid = 0.125M pKa = 4.76

Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

Q: A buffer system is set up with [HA] = 2[A-]. If pKa = 5.5, what is the pH of the buffer? %3D O A.…

A: Acidic buffer :- A mixture of weak acid and its salt with strong base is called acidic buffer. The…

Q: A buffer solution is prepared by dissolving 0.200 mol of NaH2PO4 and 0.100 mol of NaOH in enough…

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

Q: Calculate the weights of Mg(OH)2 that will dissolve in a) 250 mL of water b) 250 mL of a buffer…

A: Step-1 Let the solubility of Mg(OH)2 in 250 mL of water be ‘s’ Ksp = [S][2S]2 Ksp = 4S3 5.6 x 10-12…

Q: What is the pH of a buffer that is made by mixing 20.0 mL of 0.10 M H,CO3 and 10.0 mL of 0.20 M…

Q: A buffer solution is made that is 0.384 M in HNO2 and 0.384 M in NaNO2 . (1) If Ka for HNO2 is…

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

Q: A 25.00 mL sample of methanoic (HCHO2, Ka = 1.8 x 10-4) is titrated to the equivalence point using…

Q: What ratio of [A']/[HA] would be needed to prepare a buffer solution with a pH of 2.75 if the K, for…

A: Given: The pH of the buffer = 2.75 The Ka for HA = 4.0 × 10-4 We have to calculate the ratio of…

Q: You want a buffer solution, and you choose the following acid and conjugate base: carbonic acid,…

Q: What is the pH of a buffer that is 0.120 M in HA and 0.080 M in KA? For HA, K, = 1.8x104. О 3.57 O…

A: To find the pH of buffer solution, determine which component is the acid and which the base is and…

Q: Ethyl orange, an indicator, has a Ka of 2.0 x 10–4. The protonated form is red and the deprotonated…

A: Given : Ka = 2 x 10-4 thymol orange is an acidic indicator.

Q: Choose the best buffer system to maintain the pH at 7.00. O Acid Z and NaZ, K, = 8.0 x 10-9 O None…

Q: A 24.84 mL aliquot of a weak acid has a concentration of .58 M. It will be titrated with .32 M NaOH,…

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

Q: Calculate the concentration of free Zn2+ ion at equilibrium when 1.58x10-2 mol zinc sulfate is added…

A: Each zinc sulfate, ZnSO4 produces 1 Zn2+(aq) ion Hence moles of Zn2+(aq) ion added to 1.00 L…

Q: If a 40 mL sample of 0.200 M Hypochlorous acid (K, 2.9 x 10 ) is titrated with a 0.500 M NaOH…

A: Introduction-

Q: What is the pH of an HOBr/OBr- buffer solution prepared by adding 4.00 g of NaOBr to 300.0 mL of a…

A: Introduction : We have to calculate pH .

Q: Phosphoric acid is a triprotic acid (Kal = 6.9 × 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To…

A: We have to calculate pka and pH

Q: A 25.0 ml sample of 0.100 M lactic acid (weak acid) (HC3H5O3, Pka-3.86) is titrated with 0.100M NaOH…

Q: the volu me relmadIIs CUnStunt. Istu. Use the Henderson-Hasselbalch equation to calculate the pH of…

A: Solution, which resist in pH change value upon addition of small amount of strong acid or base (less…

Q: What is the pH of a buffer solution of 0.0025 M CH 3CO 2H and 0.00125 M CH 3CO 2Na? ( K a = 1.8 × 10…

A: Henderson-Hasselbalch equation Henderson-Hasselbalch equation explains the relationship between pH…

Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

A: Answer :- pH = 1.845…

Q: If a 30 mL sample of a 0.500 M containing a weak acid (K, = 9.5 x 10 8) is titrated with a 0.200 M…

A: Given that: Concentration of weak acid HA = 0.500M Volume of weak acid solution = 30ml Ka of weak…

Q: What is the solubility of magnesium hydroxide in a solution buffered at pH 8.95? K„ (Mg(OH)2) = 1.8…

A: Concentration of OH- can be calculated as follows:

Q: A buffer solution is prepared by dissolving 27.22g of KH2PO4 and 3.37g of KOH in enough water to…

A: KH2PO4 + KOH = K2HPO4 + H2O So, KH2PO4 and K2HPO4 acts as acid and salt made from strong base with…

Q: If [HSO4 ] = .7 M, what [SO42-] is needed to make a buffer of pH 2.2? 0.443 M 0.31 M O.217 M O 2.92…

A: According to your option, the exact answer is not matched. If we choose the option then the close…

Q: Calculate the pH of a buffer solution that is 0.250 M in HCN and 0.170 M in KCN. For HCN, Ka = 4.9 *…

A: Given: The molar concentration of acid(HCN)= 0.250 M The molar concentration of conjugate…

Q: A buffer is prepared by combining 25 mL of 0.50 M NH3(aq) with 25 mL of 0.20 M HCl. What is the pH…

A: Given : Concentration of NH3 = 0.50 M Volume of NH3 solution = 25 mL = 0.025 L…

Q: Calculate the pH of a buffered solution that is prepared by dissolving 0.3 mol of NaHCO3 and 0.45…

A: pH = pKa + log[salt]/[acid] Molar concentration = Number of moles of solute /volume of solution in L

Q: A buffer is prepared by titrating a 100.0 mL sample of 0.10 M NH3 with 50.0 mL of 0.10 M HNO3. What…

Q: 7. Calculate the pH of a buffered solution that is prepared by dissolving 0.3 mol of NaHCO3 and 0.45…

A: The pH of an acidic buffer solution is given by the Henderson-Hasselbalch equation as…

Q: Calculate the concentrations of acetic acid (pKa = 4.76) and sodium acetate necessary to prepare a…

Q: 15 mL of 0.01 M H3A solution is titrated with 0.03 M NaOH. Calculate the pH when the NaOH has been…

A: H3A is a triprotic acid.

Q: The pH of buffer solution that has Ka = 6.23 x 105 and 5a, = 3a, is: а. 4.43 b. 4.03 С. 4.38 d. 3.98…

A: pH = d. 3.98

Q: Calculate the pH for one liter of a solution containing 0.4 M acetic acid, CH3CO>H and 0.5 M sodium…

A: The scale which is used to determine the acidity/basicity of aqueous solution is called pH scale. It…

Q: What is the pH of a buffer solution prepared by adding 0.160 moles of HOBr to 175 mL of a 0.640 M…

A: Given data,Moles of HOBr=0.160molesVolume of Solution=175mL=0.175LMolarity of…

Q: A buffer solution is made by dissolving 0.230 moles of sodium hypochlorite in 1.00 L of 0.220 M…

Q: What is the pH of a buffer solution that contains 0.25 M HClO and 0.35 M NaClO? (pKa HClO = 7.46)…

A: Given PKa = 7.46 Concentration of HClO acid = 0.25 M Concentration of NaClO salt = 0.35 M…

Q: Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To…

Q: 20. The pH of buffer solution containing 0.2 mole/ liter of CH;COOH & 0.2 mole/I of CH;COONA has…

Q: If a 30 mL sample of a 0.500 M containing a weak acid (K, = 1.6 x 1o4) is titrated with a 0.200 M…

Concept explainers

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.

Question

A buffer solution is prepared by dissolving 0.200 mol of NaH 2PO 4 and 0.100 mol of NaOH in enough water to make 1.00 L of solution. What is the
2-
pH of the H 2PO 4/HPO 4
buffer if the K a2 = 6.2 x 10 8?
7.51
7.71
7.21
6.91
Click Save and Submit to save and submit. Click Save All Answers to save all answers.
Save All Answers
MacBook Air
DD
000
000
F10
F
F6
F7
F8
F9
F3
F4
F5
F2
)
C@
$4
2
4.
5
6
7.
8.
9-
T
Y.
U
Pn
W
G
J
K
S
HI
LL
R
%# 3m

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 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

Enough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of diluted buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of diluted buffer. (d) Compare your answers to Question 29(a)-(c) with your answers to (a)-(c) in this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity.
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
Consider sodium acrylate, NaC3H3O2. Ka for acrylic acid (its conjugate acid) is 5.5 105. (a) Write a balanced net ionic equation for the reaction that makes aqueous solutions of sodium acrylate basic. (b) Calculate Kb for the reaction in (a). (c) Find the pH of a solution prepared by dissolving 1.61 g NaC3H3O2 in enough water to make 835 mL of solution.
A 0.239-g sample of unknown organic base is dissolved in water and titrated with a 0.135 M hydrochloric acid solution. After the addition of 18.35 mL of acid, a pH of 10.73 is recorded. The equivalence point is reached when a total of 39.24 mL of HCl is added. The base and acid combine in a 1:1 ratio. a What is the molar mass of the organic base? b What is the Kb value for the base? The Kb value could have been determined very easily if a pH measurement had been made after the addition of 19.62 mL of HCl. Why?
For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than 7. (a) Equal volumes of 0.10 M acetic acid, CH3CO2H, and 0.10 M KOH are mixed. (b) 25 mL of 0.015 M NH3 is mixed with 12 mL of 0.015 M HCl. (c) 150 mL of 0.20 M HNO3, is mixed with 75 mL of 0.40 M NaOH. (d) 25 mL of 0.45 M H2SO4 is mixed with 25 mL of 0.90 M NaOH.
An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 M and pH is 4.20. a. Calculate the concentration of C6H5NH3+ in this buffer solution. b. Calculate the pH after 4.0 g NaOH(s) is added to 1.0 L of this solution. (Neglect any volume change.)
Indicate whether each of the following statements is true or false. If the statement is false, restate it to make it true. (a) The formate ion (CHO2-) concentration in 0.10 M HCHO2 is the same as in 0.10 M NaCHO2. (b) A buffer can be destroyed by adding too much strong acid. (c) A buffer can be made up by any combination of weak acid and weak base. (d) Because Ka for HCO3- is4.71011, Kb for HCO3- is2.1104.
A student dissolves 0.0100 mole of an unknown weak base in 100.0 mL water and titrates the solution with 0.100 M HNO3. After 40.0 mL of 0.100 M HNO3 was added, the pH of the resulting solution was 8.00. Calculate the Kb value for the weak base.
Calculate the mass of sodium hydroxide that must be added to 1.00 L of 1.00-M HC2H3O2 to double the pH of the solution (assume that the added NaOH does not change the volume of the solution).
A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.
Find [OH] and the pH of the following solutions. (a) 0.25 g barium hydroxide, Ba(OH)2, dissolved in enough water to make 0.655 L of solution (b) A 3.00 L solution of KOH is prepared by diluting 300.0 mL 0.149 M KOH with water.
A 0.288-g sample of an unknown monoprotic organic acid is dissolved in water and titrated with a 0.115 M sodium hydroxide solution. After the addition of 17.54 mL of base a pH of 4.92 is recorded. The equivalence point is reached when a total of 33.83 mL of NaOH is added. a What is the molar mass of the organic acid? b What is the Ka value for the acid? The Ka value could have been determined very easily if a pH measurement had been made after the addition of 16.92 mL of NaOH. Why?