Chemistry, 21.04.2020 23:07, stephaniem0216
In the past, many students have listed that the accidental addition of too much acetic acid contributed greatly to the difference between the experimental value and the accepted value. Suppose that Student A was supposed to make a 0.18 M solution by diluting 9.0 mL of 2.0 Macetic acid to 100.0 mL. The expected pH for this solution is 2.74. The K of acetic acid is 1.8 x 10
a. What would be the expected pH if a Student A accidentally diluted 9.1 mL (instead of 9.0 mL) of the acid to 100 mL?
b. If student A measured the above calculated pH, what would be the resultant K of acetic acid given that they expected the acid to have an initial concentration of 0.18M.
Answers: 3
Chemistry, 22.06.2019 19:00, montgomerykarloxc24x
Convert the temperature of dry ice, –77 ∞c, into degrees fahrenheit and kelvin.
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Chemistry, 22.06.2019 20:00, jalenevoyles
Phosphoric acid is a triprotic acid ( =6.9×10−3 , =6.2×10−8 , and =4.8×10−13 ). to find the ph of a buffer composed of h2po−4(aq) and hpo2−4(aq) , which p value should be used in the henderson–hasselbalch equation? p k a1 = 2.16 p k a2 = 7.21 p k a3 = 12.32 calculate the ph of a buffer solution obtained by dissolving 18.0 18.0 g of kh2po4(s) kh 2 po 4 ( s ) and 33.0 33.0 g of na2hpo4(s) na 2 hpo 4 ( s ) in water and then diluting to 1.00 l.
Answers: 3
In the past, many students have listed that the accidental addition of too much acetic acid contribu...
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