Case 1. Prepare 50 mL of a 0.3 acetate buffer solution withpH 5.01. Complete the table in preparing the buffer solutiona. Find the Molecular weight of the substances.b. determine the needed mass in grams of the substances toprepare the buffer solution. This will be based on yourcalculations. Follow the guide in the previous lesson(pp 1-3)c. compute pH of buffer solutionSubstancesMolecularMassNo. of molesweight, MW, in (in grams)g/mole= mass/MWNaOHHC,H,O,HCINa C,H,O,pH solution =2. How would you prepare and mixed the substances to make a50ml solutions.3. If you mixed the substances with distilled water and the pHis 7.5, how will you make the buffer solution change with adesired pH of 5.0?

Acetic acid and sodium acetate buffer is made with acetic acid and sodium acetate. In above question…

Answered: Case 1. Prepare 50 mL of a 0.3 acetate…

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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Hello can you help me answer question 2,3.a, and 3.b please? Thank you!
Do the 2nd and 3rd questions according to the table below. Indicator Acid color Color change, pH range Base color Methyl orange Red 3.1-4.5 Yellow Brome tymol blue Yellow 6.0-7.6 Blue 2) When the above-mentioned indicators are dropped into the two separate 10* M HCI solution, what will the color of solutions be respectively? A. Red, blue B. Red, yellow C. Yellow, yellow D. Yellow, blue E. Orange, green 3) When the above-mentioned indicators are dropped into the two separate 10 M NAOH solution, what will the color of solutions be respectively? A. Red, blue B. Red, yellow C. Yellow, yellow D. Yellow, blue E. Orange, green В. When the above-mentioned indicators are dropped into the 0.1 M NH3, what will the color of solution be? K, for NH3: 1x105
The following are steps that you might need to perform in order to prepare a buffer. Choose the answer that puts the steps in the correct order. A. Add enough water to reach the final volume needed. B. Mass out the solid buffer salt. C. Take the pH of the buffer. D. Add -60% of the total volume of water. E. Add acid or base to reach the desired pH. Select one: O B, D, C, E, A O B, A, C, E ⒸB, D, C, E, Cx B, D, A, C, E
2. In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question Which is 0.1186
How much of each solution is needed to prepare 1 L of buffer solution with a pH value of 9.45 using 0.3 M Na2CO3 and 0.2 M HCl. You need to take, calculate (Ka1 = 4.3 × 10-7, Ka2 = 4.69x10-11).
A buffer solution is prepared by taking 0.386 moles of acetic acid (pKa = 5.15) and 0.332 moles of sodium acetate in sufficient water to make 1.055 liters of solution. Calculate the pH of this solution. Report answer with 2 places past the decimal point.
In the spooky chemistry lab, you spot a 50mL solution of 6.0M hydrochloric acid. What is the pH of this acid? Yeouch...that sure would hurt if it spilled on you! You remember from when we learned about dilutions that adding water reduces the concentration of a solution. Sweet. You decide to add 950mL of water to the solution. What is the new pH of the hydrochloric acid solution? Ok, weird one here, but this is Honors Chem, so challenges are always welcome. Yippee. So, let’s rewind back to the 50mL solution of 6.0M HCl. Let’s say that you want to dilute this solution so that it has a pH equal to exactly 7. How much water would you need to add to it in order to achieve this goal? (HINT: This is so unrealistic...which is why no chemist would ever do it...but it’s still fun to do the math & determine why it’s so crazy!)
lues if heeded for this question. A buffer solution is 0.401 M in H½S and 0.278 M in KHS. If Ka1 for H2S is 1.0 × 10-7, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group 9 more group attempts remaining тес Not Visited 2red Зred Previous Next ent Save and Exit Cengage Learning | Cengage Technical Support MacBook Air .. R. 吕0 DII F1 F2 F3 F4 F5 F6 F7 F8 2$ & * %23
A Question 13 (1 point) Retake question *A buffer solution is prepared by adding 6.02 mL of 1.11 M HI to 192.0 mL of 0.11 M methylammine solution. The buffer is allowed time to establish. Then, 0.005 mol of a strong acid is added. What is the pH? Round your answer to 2 decimal places. Your Answer: Answer
how to calculate [H+] and [OH-] concentration values from the data table
A cvg.cengagenow.com OWLV2 | Online teaching and le. Content Flipgrid | 3ffc3c3b GRLContent OWLV2 | Online tea [Review Topics) [References) Use the References to access important values if needed for this question. The compound dimethylamine is a weak base like ammonia. A solution contains 9.81×102 M (CH3),NH," and 0.400 M dimethylamine, (CH3),NH. The pH of this solution is Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next Email Instructor Save and Exit Cengage Learning | Cengage Technical Support MacBook Ai DII DD

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