Could you explain how to do this problem step by step? I'm not sure where all of the numbers came from. 1. If 100 mls of 0.05 M NaoH is added to 700 mls of 0.15 M glycine buffer at pH 9.4, what is theresultant pH (PK1 for Gly= 2.2, Pk2=9.4)glycine .7LX.15mole/l = .105 molesNaOH.1LX.05mole/L= .005 molesGlyº.0525 molesStartAdd.005 moles NaOH -.005End.0475 moles.059MGly + H+.0525 moles+.005.0575moles.071MpH = pka + log [A-]/[HA] =9.4 +log.071/.059 = 9.5

Amino acids are biomolecules that have an ionisable amino group, an ionizable carboxyl group and an…

Answered: 1. If 100 mls of 0.05 M NaoH is added…

Curren'S Math For Meds: Dosages & Sol

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Author:CURREN

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Chapter17: Introduction To Iv Therapy

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At a pH of 7.40, the carbonic acid ratio is ________. a. 35:1 b. 4:1 c. 20:1 d. 3:1
2. A. If 100 mls of 0.03 M HCI is added to 400 mls of 0.5 M glycine buffer at pH 10.4, what is the resultant pH? (pK1 for Gly= 2.2, Pk2=9.4) Gly.4L X.5mol/L= .2 mol HCI.1LX.03mol/L = .003mol Glyº .02mol +.003 mol .023mol [HA] = .023/.5L =.046M, [A-] =.177/.5L = .354M pH = pka +log [A-]/[HA] pH = 9.4 +log.354/.046 = 10.3 [HCI] = [H+] = .003mol/.5L = .006M pH =2.2 Gly + H+ .18mol -.003mol .177mol end start B. What would the pH be if the same amount of HCl as in part A was added to 400 mls of water?
2) Calculate the pH during the titration of 20.00 mL of 0.1000 M butanoic acid (K,-1.54x10%) with 0.1000 M NaOH solution after the following additions .0 mL .10.00 mL 15.00 mL 19.00 mL .19.95 mL . • 20.00 mL • 20.05 mL . 25.00 mL
A buffer contains 0.015 mol of lactic acid (pK₁ = 3.86) and 0.080 mol of sodium lactate per liter. H₂C OH Lactic acid OH Calculate the pH of the buffer. H₂C. Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of the buffer. O OH Sodium lactate Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of pure water. O Na+ buffer pH: buffer pH change: water pH change: units units
1. How would you make 10 L of 0.3 M citrate buffer pH 2.5 from solutions of 0.4 M NaCitrate and 0.4 M citric acid? Include the amounts of all components added in mL. pKa = 3.09 2. How many grams of disodium hydrogen phosphate (142 g/mol), mL of 0.5 M HCl or NaOH, and mL of water are needed to make 500 mL of 0.15 M phosphate buffer pH 11.90? What would be the pH of this solution if it were diluted to 2 L with pure water? pKa(1) = 2.15; pKa(2) = 6.86; pKa(3) = 12.38 3. How many mL of 3 M NaOH or 3 M HCl and mL of 0.5 M acetate buffer pH 3.78 do you need to make 600 mL of a 0.02 M acetate buffer pH 5.3?
amino glycine pka is 2.4, 9.8 Calculate the most effective buffering range. if there is two pka, since there are 2 buffer region, is the buffering range 1.4~3.4 and 8.8~10.8? i would like to know the correct answer and detailed solution/reason.
1. Calculate the pH of the following solutions: A. [H+] = 1.36 x 10-9 M В. [ОН] —D 3.86 x 10-8 М 2. Calculate the pOH of the following solutions: A. [OH-] = 8.6 x 10-8 M В. рH %3D 3.2 3. What is the pH of a buffer prepared by mixing 100 ml 0.050 mM NAH2PO4 and 25 ml 0.075 mM Na2HPO4? (рКa1%32.2; рКо23 7.21; pКаз312.7)
You just made a 1.5M permanganate solution. What concentration is your potassium permanganate solution in percent? "K: 39.10 g/mole" "Mn: 54.94 g/mole" "O: 16 g/mole" "MW of KMnO4 is 158.04 g/mole" O a. 0.24% Ob. 20.1% O c. 15.8% O d. 23.7% O e. 2%
1. (a) Perform the calculations required to prepare 100ml of 0.20M sodium acetate buffer of pH 5.40 if you are given a bottle of sodium acetate (M.W = 82) and a bottle of concentrated hydrochloric acid (Normality = 11.M). The pKa of acetic acid is 4.80. (b) After the calculations, prepare the buffer. Check the pH of your reparation and comment on your results. 3. Prepare 1:1, 1:4, 1:10, and 1:100 dilutions of your buffer and obtain pH readings for them. Plot on a graph paper pH against buffer concentration. Explain the shape of the graph.
At what pH does a lysine solution exhibit the highest buffering capacity? (Lysine pKas: pk1 = 2.2, pK2 = 8.95, pK3 = 10.5) %3D O рH 12.1 О рH 9.72 O pH 5.67 pH 8.95
You need to prepare an acetate buffer of pH 5.43 from a 0.621 M acetic acid solution and a 2.95 M KOH solution. If you have 730 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.43? The pKa of acetic acid is 4.76. Be sure to use appropriate significant figures.
1. How many moles of acetate are there in a 200 mL 0.20 M acetate buffer pH 4.95? pKa = 4.76 2. In a solution of pH 4.76, containing both acetic acid and acetate, what can you say about the concentrations of acetic acid and acetate present?

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