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Calculation of Phosphate Buffer Solution using Henderson-Hasselbach equation
Given:
pH: 7.40
Mass of KH2PO4: 2.13 g
Molar mass of KH2PO4: 136.086 g/mol
Mass of K2HPO4: 4.24 g
Molar mass of K2HPO4: 174.3 g/mol
Volume: 250 mL
Step by step
Solved in 3 steps
- A solution contains a mixture of NaCO3 and NaOH. Using phenolphthalein indicator 25 mL of mixture required 19.5 mL of 0.995 M HCI for the endpoint. With methyl orange, 25 mL of solution required 25 mL of the same HCl for the endpoint. Calculate grams per liter of NazCO3 in the mixture. A) 23 B 11 78 (D) 360.2061 grams of an unknown organic acid was dissolved in about 50 mL of water in a 250 mL Erlenmeyer flask and titrated against 0.1000 M NaOH solution using bromothymol blue indicator. 15.56 mL of titrant was used to achieve end point. Calculate the Neutralization Equivalent. Write answer with two decimal places only. No units please.What is the volume of HF (ideal gas at 1 atm and 25°C) required to be bubbled into 250 ml distilled water to reach pH 2.50? You may assume that all the gas dissolves in the water and use pKw=14. Given: pKb (F') = 10.83. 1) 0.150 L p) 0.050 L E) 0.018 L d) 0.090L e) 0.100 L
- What is the volume of HF(g) (ideal gas at 1 atm and 25°C) required to be bubbled into 250 ml distilled water to reach pH 2.50? You may assume that all the gas dissolves in the water and use pKw=14. Given: pKb (F') = 10.83. %3D: How would you prepare a liter of "carbonate buffer" at a pH of 10.10? H2CO3 > H* + HCO3 Ka = 4.2 x 10 HCO3 +> H* + co3 2 Ka = 4.8 x 10-11 13 buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution 2nobuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution 13 buffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1- L solution 2nd buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solutionThe titration of Na₂CO3 (H₂CO3 has a pka1 = 6.37 and pka2 = 10.32) against HCl(aq) is depicted below: pH B V₁ V₂ mL HC1 E F a) Identify the major species in solution at points A - F. b) For the titration of 25.00 mL of 0.100 M Na₂CO3 against a 0.100 M HCl solution: i) calculate V₁ and V₂ ii) calculate the pH at points A - E. Note: points B and D are halfway points to equivalence.
- I euucalion.WIley.com/wasjul/V2/assessment-player/index.html?launchld=584c6e27-1041-4ce9-a7cb-8c9f8c0c154e#/question/1 A chemist needed an aqueous buffer with a pH of 3.90. Part a Your answer is correct. Would formic acid and its salt, sodium formate, make a good pair for this purpose? Formic acid and its salt, sodium formate would make a good pair for this purpose. O Formic acid and its salt, sodium formate would not make a good pair for this purpose. eTextbook and Media Attempts: 1 of 15 used Part b Your answer is correct. What mole ratio of the acid, HCHO2, to the anion of this salt, CHO,, is needed? mol HCHO, initial 0.70 mol CHO2 initial Hint Attempts: 1 of 15 used Part c How many grams of NaCHO2 would have to be added to a solution that contains 0.27 mol HCHO,? m(NaCHO2) = iVer Historial Favoritos Perfiles Pestaña Ventana Ayuda - Ultra EExperiment 7 - Google Docs G If the pH of a solution is measu X m/document/d/1HGxPrB1Rldlte19cxRUUI2Hoyd-VGYvpF2uipe950iE/edit Format Tools Add-ons Help Last edit was 3 minutes ago Normal text Arial 11 + BIUA 1 | ... 4. 7 C. Effect of Acids and Bases on the pH of a Buffer Solution C1. Effect of an acid on the pH of a buffer solution pH after adding 5 pH after adding Is the tested solution a Initial pH Solution Used Change in pH drops of HCI additional 5 drops of HCI buffer? Yes or No water 6.98 4.05 2.54 2.88 1.95 0.1 M KCI solution 6.40 pH 12 buffer solution 11.98 11.97 11.54 pH 1 buffer solution 2.05 1.85 1.63 C2. Effect of a base on the pH of a buffer solution Solution Initial pH pH after pH after Change in Is the testedWhat is the percentage of total acid expressed as acetic acid in a sample of vinegar if 4.0g of vinegar requires 29.5ml of 0.153N KOH for an endpoint with phenolphthalein indicator? (molar mass of acetic acid: HC2H3O2 = 60.05g/mol a. 3.995% b. 6.776% c. 8.650% d. 12.68%
- How many MILLILITERS of lactic acid and GRAMS of sodium lactate must be added to 1L of water to produce a solution with pH 3.9 and a total solute concentration of 1 mM? (MW Salt = 112.06; MW Acid = 90.08)Given are the values of a titration experiment of lake water: H2SO4 volume= 25ml H2SO4 diluted to:- 10% Volume of NaOH :- 0.0303L NaOH mil in volume:- 0.00455 mol Base to Acid: - 2:1 What is the concentration of Sulfuric acid (H2SO4) in the sample of lake water?A diprotic base (B) has pK, values of 3.36 (pKpi ) and 6.72 (pKg2). Which of the equalities is true when the pH is 7.28? Which of the equalities is true when the pH is 10.64? [BH*| = [B] [BH3*1= [BH* | O IBH; *1 = [B] O IBH;*| = [BH* ] [BH*] = [B] O IBH;*| = [B] What is the predominant species of B at pH 4.37? What is the predominant species of B at pH 9.10? BH;* BH* BH+ в В BH?* What is the predominant species of B at pH 12.77? В BH3* BH*