pKa = 0.52
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What is the pH of a solution containing 0.30 M HCOOH and 0.52 M HCOOK? How do i get the pKa?? I know its 3.77 but how?? Help! Edited; Nvm. figured it out, thanks
What is the [OH] in a solution that has a pH of 12.80? Given the following pKa values, which is the strongest acid of those listed in the answers? HCIO 2 (pKa = 2.00) CCl3COOH (pka = 0.52) HIO3(pka = 0.77)
1) How would you make 300 ml of a 0.1 M sodium phosphate buffer, pH 7.0 (pKa = 7.2) phosphate dibasic (the conjugate base). 2) What are the concentrations of acetate and acetic acid in a 0.2 M acetate buffer pH 5.3? The pKa for acetic acid is 4.76. 3)You have 100 ml of 0.1 M acetate buffer pH 5.2 (pKa 4.76). You add 10 ml of 0.1 M NaOH. Calculate the resulting change in pH and the buffering capacity...
Describe how you would prepare one liter 0.1 M phosphate buffer, pH = 2.5, given 0.1 M phosphoric acid and solid NaH2PO4.2H2O. pKa= 4.75
Question 14 (1 point) Calculate the pH of a buffer that is 0.268 M HC2H302 and 0.322 M LIC2H302. The Ka for HC2H302 is 1.8 x 10-5 4.72 4.82 O926 4.74 4.60
Determine the [H3O+], Ka, pKa and pH 01 each: 0.052M HI 0.075 M H2SO4 0.25 M HNO3 0.07 M HNO3 0.0250 M HCLO4 a solution that is 1.25M, H2SO4 by mass assumes a density of 1.06 g/ml for the solution mixture of acids containing 0.096 M In HI and 0.52 M in HCl mixture of acids containing 0.150 M ln HF and 0.075 M HNO3 mixture of acids containing 0.060 m ln HBr and 0.025 M HClO4
Describe how would you prepare 500.0 mL of buffer with pH = 9.08 and [HA] + [A−] = 0.10 M using the following reagents available to you in the stock room and any appropriate glassware. Available: NH4Cl (F.W. = 53.5) Ka = 5.5×10−10 pKa = 9.26 6.00M HC2H3O2 Ka = 1.8×10−5 pKa = 4.74 NaH2PO4•H2O (F.W. = 137.99) Ka = 7.4×10−8 pKa = 7.13 3.00M NaOH Deionized H2O 1) Pick the correct weak acid. 2) Solve the Henderson-Hasselbalch equation for...
Calculate the approximate pH of an aqueous solution of H2S , 0.05 M, and H3PO4, 0.21 M at 25°C. (Note: consider one decimal place for the pH answer.) pKa H2S/HS- = 7.02, pKa HS-/S2- = 13.99 pKaH3PO4/ H2PO4- =2.15, pKaH2PO4-/HPO42-=7.15, pKa HPO42-/ PO43- =12.38
What is the pH of a 125mM solution of sodium lactate? Calculate the pH of a 0.579 M aqueous solution of Lactic Acid (pKa = 3.76) Which of the following acids, if in solutions of equal concentration, is the least acidic? a) 0.1M propanoic acid pKa = 4.8 b) 0.1M octanoic acid pKa = 4.89 c) 0.1 M uric acid, pKa = 3.89 d) 0.1 M formic acid pKa = 3.75 e) All of these acids are equally acidic because...
Please explain to me how I solve this Calculate the pH of a 0.2 M acetate buffer (pKa = 4.77) that contains twice as much acid as conjugate base. Calculate the pH of the solution that results following the addition of 10mL of 1M NaOH to 40mL of 1M NH_4C1 Ka = 5.62 times 10^-10