How much of your 41M TE buffer and how much water do you need to prepare 1L of a 4.9M TE solution? Round all results to 2 positions after the decimal point. show calculations
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How much of your 41M TE buffer and how much water do you need to prepare 1L of a 4.9M TE solution? Round all results to 2 positions after the decimal point.
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- Calculate the volume of concentrated ammonia (molecular weight = 17) (PH needed to prepare 100 ml of buffer solution equal to 10.0 if the final concentration of salt is 0.2 molarity. Note that the percentage of concentrated ammonia is 28% * .10-5 x and %3D its density is 0.9 g / mL and dissociation constant 1.8To prepare the buffer, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.45 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (Supply answer up to the 2nd decimal point)14. A so-called PBS buffer (phosphate buffered saline) is prepared by according to the given protocol: ● Prepare 800 mL of distilled water in a suitable container; ● Add 8 g of NaCl to the solution; Add 200 mg of KCl to the solution; Add 1.44 g of Na₂HPO4 to the solution; Add 245 mg of KH₂PO4 to the solution; Adjust solution to desired pH (typically pH ≈ 7.4); and Add distilled water until volume is 1 L. (a) Calculate the pH of the initial solution (before pH is adjusted). (b) How many moles of acid or base are required to adjust the pH to 7.4?
- 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).Answer the following questions about the titration curve shown below. a) Choose the correct words from each pair, then explain your reasoning.The sample is a [ strong / weak ] [ acid / base ].The titrant is a [ strong / weak ] [ acid / base ]. b) What is the equivalence point volume and pH for this titration? How do you know? c) A 50.0 mL sample was titrated with 0.20 M titrant to create the titration curve. Calculate the original concentration of the sample.I have a 100X stock of a buffer. I need 100mL of 1X bugger. How much biffer solution do I use and how much water?
- 1. Answer the following, use the data and plot as a reference, answer the following questions:a) What volume of 0.100 M NaOH solution is required to reach the equivalence point, at which the solution is completely neutralized?b) Briefly explain why the pH of the solution drastically increases once the titration proceeds past the equivalence point. c) The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCl titrant. Calculate the molarity of the NaOH solution. The titration reaction equation is:NaOH (aq) + HCl (aq) → NaCl (aq) + H 2O (l)SOLVE STEP BY STEP DONT USE CHATGPT 2 ml of an Fe(II) solution of 0.08 M concentration are added to two test tubes. Subsequently, 0.5 mL of HCl with a concentration of 0.35 M is added to Tube I. 0.5 mL of NaOH with a concentration of 0.27 M is added to Tube II. Calculate the pH imposed in Tube I and II. Round the result to two decimal places.Tube I pH =Tube II pH =Give typed explanation not a single word hand written otherwise leave it A student prepared a buffer solution using 60.00 mL of 0.2336 M acetic acid and 53.35 mL of 0.09330 M NaOH. Given this information, how many moles of NaOH were used to make their buffer? Report your final answer, in moles, to 5 decimal places and only include the numerical value (no units). Do not use scientific notation to answer this question.
- To prepare the buffer, a total volume of 600 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 1.5 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 2 decimal places)Write an SOP on how to make 1L of a 1M TRIS buffer solution pH 8.0. Using the template that is shown below. PURPOSE: SCOPE: DEFINITIONS AND ABBREVIATIONS: RESPONSIBILITIES: SAFETY: MATERIALS & EQUIPMENT: PROCEDURE: SUPPORT DOCUMENTS:[Review Topics] [References] Use the References to access important values if needed for this question. An aqueous solution contains 0.305 M methylamine (CH,NH,). How many mL of 0.365 M hydroiodic acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 10.600? mL Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next Save arn Email Instructor