Suppose you nad to make a buffer to keep a solution at a pH of about 4. You have several Combinations of weak acids of bases Heat you Could use to make this buffer.: their conjugate 1 Nitrous Auid ( La=7.2xy0)4sodium nitrite 2.) Phosphoric acid (Ka=71409)4 sodium di hydrogen phospate (Ka-6.6*1)sdium fluoride 3.) Hy drofleuoric acid 4.) Benzoic acid (Kas6.3410-5)4sodiume benzoàte 5) Ethanoic acidKa=1,8«11)+ adim ethancete which of the combos uould be suitable for making the haffer? Circle all coabos above that could be used to make buffer to maintain a pt of 4. 6.) which tomb0 mainta ining ould be most effective for g a pH of 4? Write the number to that combo below. cor

Suppose you nad to make a buffer to keep a solution at a pH of about 4. You have several Combinations of weak acids of bases Heat you Could use to make this buffer.: their conjugate 1 Nitrous Auid ( La=7.2xy0)4sodium nitrite 2.) Phosphoric acid (Ka=71409)4 sodium di hydrogen phospate (Ka-6.6*1)sdium fluoride 3.) Hy drofleuoric acid 4.) Benzoic acid (Kas6.3410-5)4sodiume benzoàte 5) Ethanoic acidKa=1,8«11)+ adim ethancete which of the combos uould be suitable for making the haffer? Circle all coabos above that could be used to make buffer to maintain a pt of 4. 6.) which tomb0 mainta ining ould be most effective for g a pH of 4? Write the number to that combo below. cor

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 10P

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A sufficient quantity of each of the following aqueous solutions has been made available to you: (i) 0.2M NaH2PO4; (ii) 0.1M Na2HPO4 (a) How many ml of each of these two solutions would you require to mix together in order to prepare one litre of a 0.01M phosphate buffer pH 7.2? [For H3PO4: pKa1 = 2.15; pKa2 = 6.82; pKa3 = 12.38]. (Ans. = 14.7 ml 0.2M NaH2PO4; and 70.6 ml Na2HPO4). (b) Having calculated these volumes (of 0.2 M NaH2PO4 and 0.1M Na2HPO4) required, what further steps would you take to prepare the 0.01M phosphate buffer solution of pH 7.2?
5. How would you prepare a liter of “carbonate buffer” at a pH of 10.10? H2CO3 ↔ H+ + HCO3- Ka = 4.2 x 10-7 HCO3-↔ H+ + CO3-2 Ka = 4.8 x 10-11 a 1stbuffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution b 2ndbuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution c 1stbuffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution d 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 solution
A buffer was made by mixing 0.1404 moles of HN3 with 0.1025 moles of KN3 and diluting to exactly 1 liter. What will be the pH after addition of 10.00 mL of 0.2367 M HBr to 50.00 mL of the buffer? Ka(HN3) = 1.900e-5. Note: only a portion of the original buffer is used in the second part of the problem.
Calculate the pHpH of the buffer that results from mixing 57.9 mLmL of a 0.278 MM solution of HCHO2HCHO2 and 17.1 mLmL of a 0.535 MM solution of NaCHO2NaCHO2. The KaKa value for HCHO2HCHO2 is 1.8×10−41.8×10−4. Express your answer to two decimal places.
1. A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer? 2. Data in the table below were collected at 25°C for the following reaction:2 I–(aq) + S2O82–(aq) I2 (aq) + 2 SO42-(aq) a) Determine the rate law for the reaction. b) Calculate the rate constant, giving the correct units for k.
The carbonate anion is known to be hydrolyzed as shown in the figure. Since Ka1 = 1.45x10-7, Ka2 = 4.7x10-11 and KçBaCO3 = 5.1x10-9, calculate the solubility of BaCO3 salt at pH = 8 and pH = 12 depending on the pH value.
A. What is the pH of a 350 mL buffer containing 0.125 mol HCOOH and 0.150 mol HCOONa? Ka=1.70x10-4B. Propionic acid, CH3CH2COOH, has a Ka of 1.3x10-5 M. What mass of CH3CH2COONa would have to beadded to 1.00L of 0.500M propionic acid for a resulting solution of pH=5.00?
to prepare the buffer in the previous problem, 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: M1V1=M2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (Write your answer in 2 decimal places without the unit).
To prepare the buffer in the previous problem, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.99 M. (Remember the lesson on dilution: M1V1=M2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (Write your answer in 3 decimal places without the unit). PREVIOUS PROBLEM:
For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities. (If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.) fill in the blank 1 1. copper(II) carbonate A. AlPO4 fill in the blank 2 2. calcium hydroxide B. PbCrO4 C. PbBr2 D. PbI2 Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water. copper(II) carbonate calcium hydroxide Ksp = Ksp =
Prepare 1.0 L of 0.2 M citrate buffer, pH 5.3. Assume the availability of crystalline citric acid (FW 210), monosodium citrate (FW 214), disodium citrate (FW 236), trisodium citrate (FW 258), and 1.0 M NaOH. Citric acid pka1 = 3.10, pka2 = 4.75, pka3 = 5.40
A buffer is prepared using Lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm^3 of the 0.500 mol.dm^-3 HLac solution is mixed with 0.300 mol.dm^-3 NaLac solution to prepare the buffer. Ka for lactic acid(HLAc) is 1.4×10^-4 A) calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer