Can someone show me how to do this? The weak acid of vinegar, acetic acid, has a pKa value of 4.8. Determine the ratio of the acid form to the base form(i.e., determine [HA)/[A-]) at pH 6.0.
pH = 6.0
pH = 4.8
henderson hasselbalch equation
pH = pKa + log [A- / HA]
6.0 = 4.8 + log [A- / HA]
1.2 = log [A- / HA]
[A- / HA] = 10^1.2
= 15.85
[HA /A-] = 1/15.85
= 0.063
the ratio of the acid form to the base form = 0.063
Can someone show me how to do this? The weak acid of vinegar, acetic acid, has...
2. A particular sample of vinegar has a pH of 2.95. Part A If acetic acid is the only acid that vinegar contains (Ka=1.8×10−5), calculate the concentration of acetic acid in the vinegar. Express your answer using two significant figures. 3.A new potential heart medicine, code-named X-281, is being tested by a pharmaceutical company, Pharma-pill. As a research technician at Pharma-pill, you are told that X-281 is a monoprotic weak acid, but because of security concerns, the actual chemical formula...
with at least 10 data points
choose a weak acid (such as formic acid, acetic acid, benzoic acid) and calculate/plot a titration curve for a 0.1 M solution of this acid with strong base using Excel. Do the same for a weak base (ammonia, TRIS) titrated with strong acid Prepare a titration curve (pH vs. equivalents strong base added if you choose a weak acid to be titrated) in which you plot at least 10 data points starting from 0-equiv...
Acetic acid is a weak acid found in vinegar. The pure substance has a density of 1.049g/mL. What is the mass of 24.5 mL of acetic acid? Show all work
Question 39 1 pts A weak acid (HA) reacts with a weak base (B) to form the conjugate base of the acid (A) and the conjugate acid of the base (B-H the pKa of HA was 4.8 and the pKa of BH* (i.e., the pKabH of B) was 9.4, what would be the value of the equilibrium constant for the above reaction to the nearest ones? Obviously, by expressing the answer to the nearest ones, we are using too many...
PART A: A particular sample of vinegar has a pHpH of 2.95. If acetic acid is the only acid that vinegar contains (Ka=1.8×10−5), calculate the concentration of acetic acid in the vinegar. Express your answer using two significant figures. PART B: A new potential heart medicine, code-named X-281, is being tested by a pharmaceutical company, Pharma-pill. As a research technician at Pharma-pill, you are told that X-281 is a monoprotic weak acid, but because of security concerns, the actual chemical...
How do you calculate the pH of a solution containing a weak acid or a weak base? Please write down the general formula for finding the H3O+ ion concentrations in case of a weak acid Please explain the common-ion effect in terms of Le Châtelier. You might want to use the general chemical equation for an acid ionization HA + H2O ↔ A- + H3O+ to help you explain the phenomenon. How do you calculate the degree of ionization? Please...
can someone plese help me?
Consider the weak acid, CH3CO2H, acetic acid. Provide its ionization reaction:
Vinegar is a solution of acetic acid. Acetic acid has a 1:1 ratio when reacted with NaOH. a. Suppose that the molarity of acetic acid in vinegar is 0.5 M, how many grams of acetic acid are present in the 5 ml of vinegar solution used in the titration? (molar mass of acetic acid = 60 g/mol). b. If vinegar has a density of 1.01 g/mol. Calculate the % of acetic acid in vinegar by mass.
I need to know the % output when :
weak acid( pKa=6) is in pH of urine at 6 and pH or urine at
8.
Also the weak base (pKa 7) in pH of urine at 6 and pH or urine
at 8.
Effect of urine pH on delivery route: Weak organic acids and bases can reach the luminal fluid (the filtrate, the primary urine) either by glomerular filtration in Bowman's capsule or by secretion in the proximal tubule. In...
Can someone please help me with these questions? Please write out the steps as well so that i understand it best. Thank you! 1. A solution of acetic acid is 28.5% deprotonated. What is the pH of the solution if the pKa for acetic acid is 4.76? 2. 20 mL of 2.00 M HNO3 is added to 100 mL of 0.15 M NaOH. What is the final pH of the solution? 3. A solution of carbonic acid (H2CO3) has a...