PLEASE COMPLETE ALL ANSWER. SHOW ALL WORK.


PLEASE COMPLETE ALL ANSWER. SHOW ALL WORK. For questions 10 and 11. You need a buffer...
please answer 23 and 24
*please show all work and calculations *
given temperature foart em to reach equilibrium e con 15) Pure Solic and pure liquide are excluded from equilibrium constant pre Cheric £69 kg 19) If a reaction is endothermic, the reaction temperature results in an ineren 20) A solution of ammonia is 2.0% ionized at 25.0 °C. What was the original concentration in M) of the ammonia solution? The Kb at 25.0 °C for ammonia is 1.8...
(4) 6 pts. A buffer contains 0.500 M of Formic acid (HCHO,) and 0.500 M of sodium formate (NaCHO2). Formic acid is a weak acid that dissociates in water as following: HCHO2 (aq) + H20 (1) =H30+ (aq) + CHO2 (ag) The equilibrium constant: Ks = ([H30+1X[CH02:])/[HCH02] =1.8 x 10-4 Calculate the pH of the buffer solution.
1a. Which weak acid should be used to create a buffer at pH= 3.1 "Chloroacetic Acid, CClH2O2H, Ka = 1.36×10–3" "Lactic Acid, C3H6O2, Ka = 1.38×10–4" "Acetic Acid, CH3O2H, Ka = 1.75×10–5" "Carbonic, H2CO3, Ka = 4.30×10–7" "Hypochlorous Acid, HOCl, , Ka = 3.50×10–8" "Hypobromous Acid, HOBr, Ka = 2.00×10–9" 1b. How many grams of sodium formate (NaCHO2) need to be dissolved in 151 mL of a 1.12 M formic acid (pKa= 3.75) solution, so that the concentration of formate...
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7. You need to make a buffer to keep a solution at a pH of 2.50. You have several combinations of weak acids and their conjugate bases to choose from. 1. Chloroacetic acid (K4 = 1.40 x 103) and sodium chloroacetate 2. Formic acid (Ka = 1.77 x 10-4) and sodium formate 3. Iodic acid (Ka = 1.60 x 10-1) and sodium iodate 4. Phosphoric acid (K. = 7.52 x 10-3) and sodium phosphate 5. Propionic...
You work in a research lab with a chemist who asks you to make 500.0 mL of a formic acid/sodium formate buffer solution with pH = 4.10. Formic acid is HCOOH(aq); sodium formate is NaHCOO(s) and is soluble in water. The total concentration of formic acid + formate ion in the buffer is to be 0.120 M. Ka(HCOOH) = 1.77 × 10–4 (pKa = 3.75). In the storeroom, there are the following reagents: (i) solid sodium formate, (ii) a 3.00...
QUESTION 3 To make a buffer of formic acid (Ka = 1.8 x 10-4)
with a pH = 4.00, what ratio of formic acid to sodium formate is
required? (Notice that I am asking for the ratio of acid to base,
not base to acid!)
a) 1.25
b) 0.56
c) 0.82
d) 1.87
QUESTION 4 If you find that you need an acid to base ratio of
4.23 and you are using 50.00mL of a 1.00M acid solution, what
volume...
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17. Calculate the pH of a solution composed of 0.050 M formic acid (K.- 1.8 x 10") and 0.35 M sodium formate. (5 points)
7. You need to make a buffer to keep a solution at a pH of 2.50. You have several combinations of weak acids and their conjugate bases to choose from. 1. Chloroacetic acid (K. = 1.40 x 10") and sodium chloroacetate 2. Formic acid (K= 1.77 x 104) and sodium formate 3. Iodic acid (K-1.60 x 10-') and sodium iodate 4. Phosphoric acid (K, = 7.52 x 10%) and sodium phosphate 5. Propionic acid (K, - 1.34 x 10 %)...
can you please answer 1,2, and 3 and show the steps
1. Calculate the pH of a buffer solution made by adding 20.0 mL of 0.200 M acetic acid solution with 10.0 mL of a 0.200 solution of sodium acetate. K, for acetic acid is 1.8 x 109. Assume the total volume is 30.0 mL. 2. Calculate the pH of a buffer solution made by mixing 10.0 mL of 0.20 M ammonia with 15.0 mL of 0,15 M ammonium chloride...
(Please show work) A 100.0 mLbuffer solution is 0.250 M in acetic acid (CH3COOH) and 0.250 M in sodium acetate (CH3COONa). [Acetic Acid (CH3COOH) Ka = 1.8 x 10-5] a)What is the pH of this buffer solution? b)What is the pH after addition of 0.0050 mol of HCl? c)What is the pH after addition of 0.0050 mol of NaOH?