A buffer solution is composed of 1.324 g of KH2PO4 and 4.362 g of NazHPO4. (K, for dihydrogen phosphate ion is 6.2 × 10-8.) a. What is the pH of the buffer solution? pH = b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass = b)

A buffer solution is composed of 1.324 g of KH2PO4 and 4.362 g of NazHPO4. (K, for dihydrogen phosphate ion is 6.2 × 10-8.) a. What is the pH of the buffer solution? pH = b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass = b)

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A buffer solution is made that is 0.498 M in HNO2 and 0.498 M in KNO2. If Ka for HNO2 is 4.50 x…

Q: What is the pH of a 75.0 ml of a 0.1 M pyridine (C5H5N) solution (Kb= 1.7 x 109) when 100.0 mL of a…

Q: A solution contains 1.42×10-2 M aluminum acetate and 7.14x10-3 M lead nitrate. Solid sodium…

A: Given, The concentration of the aluminum acetate = 1.42×10-2 M The concentration of the lead nitrate…

Q: Create 50 mL of a pH = 10.00 buffer solution using solid bicarbonate (NaHCO3, baking soda, pKa =…

A: Given: Mass of NaHCO3 taken = 1 g. And pH of the solution = 10.00

Q: A buffer must be a pH of 10.00 and 750 mL total volume. We have 20 L of 0.20 M NaHCO3 and solid…

Q: The weak base Mg(OH)2 is weak because it is only partially soluble in water at 25 °C (Ksp =…

Q: What volumes of 0.200 M HNO2 and 0.200 M NaNO2 are required to make 500. mL of a buffer solution…

Q: You want to make a 500.0 mL of 0.080 M of phosphate buffer pH = 7.90 from Na2HPO4 and NaH2PO4…

Q: A student forgot to label two bottles of aqueous base. One contained KOH and the other C6H5NH2. What…

A: KOH is a strong base and the other C6H5NH2 is a weak base. Strong base is 100% ionized in aqueous…

Q: i. First, identify the acid. It's either H2PO41 or HPO42. The acid is because it has the most acidic…

A: Answer-1 H2PO4- H2PO4- because it has more number of acidic hydrogens, that's why it will lose it…

Q: Part A: A 252-mL buffer solution is 0.420 M in ammonia (NH3) and 0.303 M in ammonium chloride…

A: We would use Henderson Hasselbalch equation to calculate initial pH. Then , HBr which is a strong…

Q: A chemistry graduate student is given 450. mL of a 0.70M methylamine (CH3NH₂) solution. Methylamine…

A: The objective of the question is to calculate the mass of .

Q: Consider the titration of 300.0 mL of 0.450 M NH 3 ( K b = 1.8 × 10 –5) with 0.450 M HNO 3. How…

A: Given: Concentration of NH3 = 0.450 M Volume of NH3 solution = 300.0 mL And concentration of HNO3 =…

Q: A chemistry graduate student is given 500. mL of a 0.30M chlorous acid (HC102) solution. Chlorous…

A: To solve this problem, we need to use the Henderson-Hasselbalch equation, which relates the pH of a…

Q: Determine the pH of a solution that is 0.45 M CH3COOH and 0.10 M CH3COONa. 1

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

Q: A chemistry graduate student is given 450. mL of a 1.80M methylamine (CH3NH2) solution. Methylamine…

A: Step 1:Solution of weak base methylamine (CH3NH2) and its conjugate base (CH3NH3Br) is a buffer.…

Q: A buffer is made by mixing 40.00 mL of a 0.100 M solution of the fictitious acid HA (pKa = 5.11)…

A: Given,Molarity of fictitious acid, HA = 0.100 M ( pKa = 5.11 )volume of HA = 40.00 mLMolarity of…

Q: 2. What is Buffer capacity (Bmax)?

A: Buffer capacity is a measure of the efficiency of a buffer, in resisting changes in pH.

Q: 1. What is the pH of a solution containing 0.20mol of NH4Cl and 1.5mol of NH3? Kb = 1.8 x 10-5

A: Detail

Q: a A chemistry graduate student is given 450. mL of a 1.40M chlorous acid (HCIO2) solution. Chlorous…

A: Given: Vbuffer=450.mL;[HClO2]=1.40M;pH=1.94;Ka=1.1x10−2massNaClO2=???g;MNaClO2=90.44g/molStep…

Q: A 349-mL buffer solution is 0.372 M in nitrous acid (HNO2) and 0.346 M in sodium nitrite (NaNO2).…

Q: A buffer solution contains dissolved C₆H₅NH₂ and C₆H₅NH₃Cl. The initial concentration of C₆H₅NH₂ is…

A: A solution which is a mixture of weak acid and its conjugate base is known as buffer. For…

Q: 4.b A buffer contains the weak acid HAHA and its conjugate base A−A−. The weak acid has a pKapKa of…

A: If you add base to a buffer, the ph must increase slightly If you add acid to a buffer, the ph must…

Q: Part 1: A buffer system is set up with [HA] = 0.550 M and [A-] = 0.460 M in 1.0 L of aqueous…

Q: A buffer solution is made that is 0.386 M in HNO2 and 0.386 M in KNO2. If Ka for HNO2 is 4.50 ×…

A: Interpretation - The pH of the buffer solution and net ionic equation for the reaction that occurs…

Q: Consider the titration of H2SO4 with NaOH. A 30.0 L sample of H2SO4 requires 0.090L of 0.100 M NaOH.…

A: The acid base titration reaction of H2SO4 and NaOH is, H2SO4 + 2 NaOH ----> Na2SO4 + 2H2O Here we…

Q: A buffer was prepared by adding 7.50 moles K2HPO4 and 9.60 mol KH2PO4 to a 1.0 L solution. Ka2 = 6.2…

A: the mentioned buffer is an acidic where KH2PO4 is the weak acid and K2HPO4 is the salt component.

Q: a. What is the pH of a buffer solution that is 0.18 M NH3 and 0.18 M NH? Ki for NH3 is 1.8 x 10-8.…

A: a.) To calculate pH, we would use Henderson Hasselbalch equation. b.) First we need to calculate…

Q: buffer solution is made that is 0.485 M in HNO2 and 0.485 M in NaNO2 . If Ka for HNO2 is 4.50 x…

Q: decimal places If the pH calculated in b. was the blood pH of an actual patient, would you say this…

Q: Imagine you want to want to make a phosphate buffer in the lab that resembles the bloods phosphate…

A: Here we are required to find the buffer of the solution.

Q: with a 0.2500M solution of NaOH. The p K of butanoic acid is An analytical chemist is titrating…

Q: solution. Methylamine is a weak base with K = 4.4 x 104. What mass of A chemistry graduate student…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: A chemistry graduate student is given 450. mL of a 1.00M chlorous acid (HClO₂) solution. Chlorous…

A: We would use Henderson Hasselbalch equation to calculate the mass of NaClO2 required. First we would…

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 composed of 1.324 g of KH,PO4 and 4.362 g of Naz HPO4. (K, for dihydrogen phosphate ion is 6.2 × 10-8.)
a. What is the pH of the buffer solution?
pH =
b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a?
Mass =

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

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

Buffers 1. Determine the pH of a solution that contains 0.376 M hydrogen phosphate (HPO) and 0.468 M dihydrogen phosphate (H₂PO₂). Ka dihydrogen phosphate = 6.2 10 H_PO_ (aq)+H_O H₂O (aq) + HPO (aq) 4
Suppose you have an alkaline buffer consisting of 0.20 M aqueous ammonia (NHs) and 0.10 M ammonium chloride (NH4CI). What is the pH of the solution? 5 Calculate the pH of a 0.350 M solution of potassium phenolate, KC6H5O. Ka for phenol (CH5OH) is 1.0 x 10-10. How do the concentration/volumes of the buffer affect the buffer capacity? E.g., 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid solution with 25.0 mL of 0.10 M sodium acetate solution).
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M NaH2PO4 and 0.50 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis?
question 7!
You dissolve 0.194 g of NaOH in 2.00 L of a buffer solution that has [H2PO4] = |HPO, | = 0.188 M. What is the pH of the solution before adding NaOH? (K, for dihydrogen phosphate ion is 6.2 x 10-8.) pH = What is the pH of the solution after adding NaOH? pH =
1. Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid (HAc). Ka for HAc is 1.8x10 -5. What is the initial pH of the solution (before the titrant is added)?
A 400-mL buffer solution is 0.350 M in ammonia (NH3) and 0.350 M in ammonium chloride (NH4Cl).Kb(NH3)=1.76×10−5Part A:What is the initial pH of this solution? Express your answer using two decimal places.pH = 9.25 Part B:What is the pH after adding 125.0 mL of 0.100 M HBr to the initial buffer solution in Part A?Express your answer using two decimal places.pH = (not 10.26) Part C:What is the pH after adding 150.0 mL of 0.100 M LiOH to the initial buffer solution in Part A?Express your answer using two decimal places.pH = (not 8.33) --------------------------- Give the formula for tin(IV) hydroxide.
Calculate the concentration of an HCl solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)₂ to reach the titration endpoint. Mg(OH)2 + 2 HCl → 2 H₂O + MgCl₂ There is enough information to calculate the moles of base but not the moles of acid. mol b. 0.1320 i. OH-1 p. CO3² W. PO4³ a. 0.1000 h. CaCO3(s) o. H₂PO4-¹ v. H₂CO3 bb. 3.300 x 10-² hh. 2.16 x 10-6 L)(- mol Mg(OH)3)(- mol HCI c. HX j. H30+1 q. HCO3-¹ x. HCzH3Oz dd. 2 jj. 0.2000 d. Al+3 k. SO4² r. H₂S CC. 3 ii. 1.60 x 10-5 e. CO₂ 1. Mg+2 S. HS-1 y. C₂H30₂-1 ee. 1 = mol HCI mol Mg(OH)₂ M HCI f. CaF2(aq) m. C-1 t. S-2 z. 1 x 10-14 ff. 0.099536 kk. 6.600 x 10-³ g. HF(aq) n. HPO 2 u. H₂O(lig) mol Mg(OH)3 aa. 1.32 x 102 gg. 3.95 x 10-3 mol HCI
= く O Acids and Bases Calculating the composition of a buffer of a given pH 0/5 a A chemistry graduate student is given 300. mL of a 0.70 M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K = 4.9 x 10 10. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 9.48? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10 ㅁ
An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution? 2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution? 3. What is the concentration of Ag+ in solution?
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)
Titrating ascorbic acid with iodine is what type of titration? HO. HO. + 2 HI HO 3x-3x= h + HO HO OH Iodine Ascorbic Acid Dehydro-Ascorbic Acid O An acid-base neutralization titration, because iodine is a strong acid OA redox titration, because iodine acts as an oxidizing agent OA redox titration, because iodine acts as a reducing agent An acid-base neutralization titration, because ascorbic acid is a weak base