You need to make a buffer that contains 8% (w/v) of dihydrate calcium chloride. How much ANHYDROUS calcium chloride is needed to make 3.5L of the buffer with the same molar concentration?
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You need to make a buffer that contains 8% (w/v) of dihydrate calcium chloride.
How much ANHYDROUS calcium chloride is needed to make 3.5L of the buffer with the same molar concentration?
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- Enough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of diluted buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of diluted buffer. (d) Compare your answers to Question 29(a)-(c) with your answers to (a)-(c) in this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity.If you have a ka = 8.25x10^-8, what buffer system will you use? Acetic acid (HC2H302) - Acetate ion (C2H302-) Carbonic acid (H2co3) - Hydrogen carbonate ion (HCO3-) Dihydrogen phosphate ion (H2P04-) - Hydrogen phosphate ion (HPO4 2-) Hypochlorous acid (HCIO) - Hypochlorite ion (CIO-)Suppose you want to make a buffer with a pH of 6.90. Which of the following acid/conjugate base pairs should you choose? Group of answer choices HOCl and OCl- (Ka = 3.5 x 10-8) HSO4- and SO42- (Ka = 1.2 x 10-2) C6H5CO2H and C6H5CO2- (Ka = 6.5 x 10-5) HF and F- (Ka = 6.6 x 10-4)
- 4. Human blood is slightly basic in nature with a normal pH range of 7.35-7.45. The blood pH is maintained by the carbonic acid-bicarbonate buffer system, shown by the following equilibrium reaction. H2CO3 + H2O H,O* + HCO3 a) If you add a small amount of an acid to this buffer, then which component of the carbonic acid-bicarbonate buffer will react with the added acid? Explain.A chemistry graduate student is given 250. mL of a 1.40M ammonia (NH3) solution. Ammonia is a weak base with K-1.8x10 should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.17? What mass of NH, Br You may assume that the volume of the solution doesn't change when the NH4Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?A buffer is prepared with H₂CO3 and NaHCO, What is the correct net ionic equation describing what happens when a small amount of NaOH is added to the buffer? O H₂COOH (lag) HCO₂ (aq) + H₂O OHCO₂(g) + H₂O H₂COglag) + OH (ad OHCO, la-OH lag) CO2(g) + H₂O(g) O HCO, lad H₂O+laala H₂CO₂log) + H₂O
- bha A buffer prepared by dissolving oxalic acid dihydrate (H2C2O4·2H2O) and disodium oxalate (Na2C2O4) in 1.00 L of water has a pH of 5.333. How many grams of oxalic acid dihydrate (MW = 126.07 g/mol) and disodium oxalate (MW = 133.99 g/mol) were required to prepare this buffer if the total oxalate concentration is 0.241 M? Oxalic acid has pKa values of 1.250 (pKa1) and 4.266 (pKa2).Two buffers are prepared by adding an equal number of moles of formic acid (HCOOH) and sodium formate (HCOONa) to enough water to make 1.00 LL of solution. Buffer A is prepared using 1.00 molmol each of formic acid and sodium formate. Buffer B is prepared by using 0.010 molmol of each. (Ka(HCOOH)=1.8×10−4.) Calculate the pHpH of each buffer. Which buffer will have the greater buffer capacity?A student wants to make a pH 4.0 buffer solution. She decides to use a buffer made from formic acid and sodium formate (HCOONa). She adds 50.0 grams of sodium formate to a 1 L volumetric flask. The Ka of formic acid is 1.77×10-4. How many mL of 3.0 M formic acid should she add to the 1 L volumetric flask so that when the flask is diluted to the mark the pH will be 4.00?
- Suppose you want to make a buffer with a pH of 3.60. Which of the following acid/conjugate base pairs should you choose? HOCI and OCI- (K, = 3.5 x 108) HF and F- (Ka = 6.6 x 104) C6H5CO2H and C,H5CO2' (Ka = 6.5 x 10 5) HSO4 and SO,2 (Kg = 1.2 x 102)Given the Kb's of three weak bases and the Ka's of two weak acids choose the one that could be used as one of the components of a buffer solution with a pH of 6.35. 1. CH3COOH (Ka = 1.8 x 10–5) 2. NH2OH (Kb = 1.1 x 10–8) 3. CH3NH2 (Kb = 4.4 x 10–4) 4. C5H5N (Kb = 1.7 x 10–9) 5. HCOOH (Ka = 1.8 x 10–4)A butanoic acid/sodium butanoate (C3H7COOH/NAOOCC3H7) buffer is prepared to 1.14×10-2 mol L-1 C3H;COOH and 1.43×10-2 mol L-1 Na0OCC3H7. The Ka for butanoic acid is 1.5×10-5. What is the pH of the buffer solution? Part A 5.03 O 4.92 4.82 O 4.73 O 4.43
