Procedure Part A: Preparation of Solutions Sodium Bicarbonate Solution: Write procedures for preparing 50 mL of 0.1 M solution of sodium bicarbonate (Baking Soda). Use calculations to prepare solution.
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![Calculations
Henderson-Hasselbalch equation: pH= pKa + log ([A/[HA])
Buffer Capacity (Moles of H* or OH added)/(A pH)(Amount of Buffer, L)
Procedure
Part A: Preparation of Solutions
Sodium Bicarbonate Solution:
Write procedures for preparing 50 mL of 0.1 M solution of sodium bicarbonate (Baking Soda). Use calculations
to prepare solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb8391471-fe9a-4660-9fda-0c9d6446ea27%2F633f9e80-8612-4623-859a-a90b6bbe7364%2F9zdbd4h_processed.jpeg&w=3840&q=75)
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- A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelatedStudent Q prepared 50.0 mL of a buffer solution using 0.50 moles of HA and 0.50 moles of A- while Students S prepared 50.0 mL of a buffer using 0.25 moles of HA and 0.25 mole of A-. a. Do the two buffer solutions have the same or different pH? Explain b. If 1.00mL of 0.010M NaOH were added to the two buffers, would the pH of the two solutions increase or decrease? Explain. c. Which solution (Buffer Q or Buffer S) would show a smaller chanign in pH for question b? Explain.Prepare 100 mLof a 0.01 M phosphate buffer, pH 7.70, from stock solutions of 0.1 M K2HPO4and 0.2 M KH2PO4. (pKa for the weak acid = 7.20). a.Use the Henderson-Hasselbalch equation to calculate the volume of each stock solution needed. pH = pKa + log [conjugate base] / [weak acid] Make the solution and check the pH of a portion of your buffer solution using the pH meter
- Which of these statements is true? (a) If you add strong acidor base to a buffer, the pH will never change. (b) In orderto do calculations in which strong acid or base is added toa buffer, you only need to use the Henderson–Hasselbalchequation. (c) Strong bases react with strong acids, but not weak acids. (d) If you add a strong acid or base to a buffer, thebuffer’s pKa or pKb will change. (e) In order to do calculationsin which a strong acid or base is added to a buffer, you need tocalculate the amounts of substances from the neutralizationreaction and then equilibrate.Please calculate the pH of a buffer solution made up of citric acid and potassium citrate. The solution was made by dissolving 0.770 mol of sodium citrate, and 0.770 mol of citric acid in 1.5 liters of water. (Please assume the total volume of the solution is also 1.5 L) (The Ka for this system = 7.41 x 10-4) (Please answer with 3 sig. figs.)John is creating a 625 mM HEPES-KOH buffer in 250 mL volume at a pH of 8.0. what volume (in milliliters) of 5 M KOH should you use? Show all steps.
- Calculate the concentration of OH- and the pH of a solution that is 0.20 M in aqueous NH3 and 0.10 M in NH4Cl using the Henderson-Hasselbalch equation. ** Need asap pls. Thanks.part a: A 0.500-L buffer solution was made with 0.25 M NH3 (Kb = 1.8 × 10-5) and 0.40 M NH4Cl. What would be the pH of this solution? part b: How many milliliters (mL) of 19.00 M NaOH are need to adjust the pH of this buffer to pH 10.00? Please answer part bIf applicable, ensure you include all units and formulas used and you follow significant figure rules. 4. What is the pH of a buffer made from 0.42 M H3BO3 and 0.32 M H2BO3-, if the Ka for H3BO3 is 7.3 x 10-10 ? (use 2 decimal places for pH) 5. Write a balanced chemical equation for the following reactions: **You do not need to indicate s, l, g or aq.** a) potassium carbonate and hydrobromic acid b) solid magnesium metal and phosphoric acid 6. If 46.3 mL of a 0.794 M Ca(OH)2 solution is required to neutralize a 40.0 mL sample of HCl, what is the molarity of the acid solution? ensure you write a balanced neutralization reaction.
- 1. Refer to Appendix 6 which shows the calculations involved in determining the volumes of 0.20 M acetic acid and 0.20 M sodium acetate needed to make 20.00 mL of a buffer with pH = 5.00. Study the method used: set up two equations with two unknowns; the first is the Henderson-Hasselbalch equation, the second is the fact that the volumes of HA and A− solutions should sum to 20 mL. In the Henderson-Hasselbalch equation, use the same volumes for the ratio, since the concentrations of the HA and A− solutions are the same, and the change in the ratio is due to the different volumes. Once you understand the method, use it to calculate the volumes of 0.20 M acetic acid and 0.20 M sodium acetate needed to make 20.00 mL of a buffer having pH = 4.00 and again to make 20.00 mL of a buffer with pH = 6.00. Your TA will check the accuracy of your calculations before you mix your buffer solutions. 2. Between the three buffers (pH 4, pH 5, pH 6), which will stay in the buffer region for the…For the addition of 0.1 mol/L NaOH to 25 mL of 0.1 mol/L HCl prepare a "ph curve" as follows: a) Find the PJ of the acid solution just befor the end point when 0.1 mL of base less than end point colume has been added. we are assuming that the end point equals equivalence point, therefore at the end of the titration pH = 7 b) Repeat calculation 'a' for a volume 1 mL less and 5cmL less then end point and before any base is added.(That is 0mL base added.) before end point, we assume that all the base is used up by the acid. C) Assuming you had continuied the titration past the end point, calculate the pH when 0.1 mL of base beyond end point had been added. D) repeat calculation'c' for 1 mL, 5 mL and 10 mL of base beyond end point. e) From your results, construct a ph (y axis) versus "volume of base added" graphI need help filing in this table and calculating pH and buffer capacity solve this question correctly in 5 min pls Chemicals & Reagents • pH 4.01 and pH 7.00 Standard solutions • 0.1 M Na2HPO4 (sodium phosphate dibasic) • 0.1 M KH2PO4 (potassium phosphate monobasic) • 0.1 M NaOH (sodium hydroxide)