Be sure to answer all parts.What volumes of 0.200 M HCOOH and 2.00 M NaOH would make 0.450 L of a buffer with the same pHas a buffer made from 475 mL of 0.200 M benzoic acid and 25 mL of 2.00 M NaOH?Volume of HCOOH = 0.42ICOOHVolume of NaOH =0.03X NaOH

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Answered: Be sure to answer all parts. What…

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...

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Find the pH of a 1.3x10-5 M HCI solution. 4.89 If 1 mL of 0.1 M NaOH is added to 1 L of the acid, what is the resulting pH? 3.00 How do these pH values compare to the buffer you made in part 2b? The pH of this solution has a change greater than ✓ the pH of the buffer made in part 2b of the experiment.
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?
1. A buffer is prepared using 0.522 mol of NH4CI and 0.812 mol of NH3 to make 1.00 L of solution. What is the pH of the solution after adding 0.153 mol of NaOH. Assume that the volume change is negligible. The pKa of NH4Cl is 9.26. 2. A buffer is prepared using 0.636 mol of HO2C2H3 and 0.848 mol of NaO2C2H3 to make 1.00 L of solution. What is the pH of the solution after adding 0.137 mol of HCI. Assume that the volume change is negligible. The pKa of HO2C2H3 is 4.74.
What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.13 M C6H5COOH and 0.30 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures. [H3O+] = ___× 10___MpH =____
a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF.The Ka for HF is 7.2×10-4. pH = b) Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0014 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3×10-7 Сoncentration = M c) You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH , the pH is 5.50. What is the Ka value of HA ? = d) Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. 40.0 mL pH = 50.0 mL pH =
Which of the following, if dissolved in 1.0 L of pure water, will produce a buffer solution? 0.1 mole HCL + 0.1 mole KCl 0.1 mole NaH2PO4 + 0.1 mole Na2HPO4 0.1 mole NaCl + 0.1 mole KCl 0.1 mole of H3O+ + 0.1 mole OH- I am guessing option 2, but need clarification please!
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)
Can you help me with this please
Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or base is added. Suppose that you have 105 mL of a buffer that is 0.260 M in both benzoic acid (CH₂COOH) and its conjugate base (CH₂COO¯). Calculate the maximum volume of 0.270M HCl that can be added to the buffer before its buffering capacity is lost. volume: mL
A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kp (C2H5NH2) = 4.3 x 104 Express value to three decimal places. Determine the number of moles of base that can be added before the buffer capacity is exceeded. moles base F TOOLS x10
Calculate the pHpH of the buffer that results from mixing 57.9 mLmL of a 0.278 MM solution of HCHO2HCHO2 and 17.1 mLmL of a 0.535 MM solution of NaCHO2NaCHO2. The KaKa value for HCHO2HCHO2 is 1.8×10−41.8×10−4. Express your answer to two decimal places.

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Be sure to answer all parts. What volumes of 0.200 M HCOOH and 2.00 M NaOH would make 0.450 L of a buffer with the same pH as a buffer made from 475 mL of 0.200 M benzoic acid and 25 mL of 2.00 M NaOH? Volume of HCOOH = 0.42 ICOOH Volume of NaOH = 0.03 X NaOH