Question
In: Chemistry
When you'll transfer a 35 ml solution using a 50 ml burette, what are your sources...
When you'll transfer a 35 ml solution using a 50 ml burette, what are your sources of errors?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
When you'll transfer a 35 ml solution using a 50 ml burette, what are your sources...
When you'll transfer a 35 ml solution using a 50 ml burette,
what are your sources of errors? Room temperature? Tapering end of
the burette? Any clue?
What is the pH when 50 ml of 0.040 M NaOH is mixed with 50 ml...
What is the pH when 50 ml of 0.040 M NaOH is mixed with 50 ml of
0.040 M HN3 (Ka= 1.9*10^-5)
After we transfer a 100 ml sample of the HCl solution into a 125 ml erlenmeyer...
After we transfer a 100 ml sample of the HCl solution into a 125
ml erlenmeyer flask, we add 50 ml of distilled water and 3 drops of
phenolphthalein indicator solution. The resulting solution requires
44 mL of 0.125M NaOH solution to reach the end point.
Calculate the number of Moles NaOH needed., and the Molarity of
HCl.
Please help... I somehow got a 284 Molarity solution...
The following buffer was prepared: 50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of...
The following buffer was prepared:
50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of 2.0 M
methylamine hydrochloride (CH3NH3Cl) solution. The Kb for
methylamine is 4.4 x 10-4.
What is the pH of the resulting solution after adding 100 ml of
1.0 M HCl to the original buffer solution?
a) 11.12 b) 10.64 c) 12.32 d) 0.48 e) 5.32
The following buffer was prepared: 50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of...
The following buffer was prepared:
50. mL 2.0 M methylamine (CH3NH2) solution
and 50. mL of 2.0 M methylamine hydrochloride
(CH3NH3Cl) solution. The
Kb for methylamine is 4.4 x
10-4.
A. What is the pH of the resulting solution after adding 200 ml
of 1.0 M HCl to the original buffer solution?
a)11.12
b)
10.64
c)
12.32
d) 0.48
e) 5.32
B.What is the pH of the resulting solution after adding 50 mL of
1.0 M KOH to the...
The following buffer was prepared: 50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of...
The following buffer was prepared: 50. mL 2.0 M methylamine
(CH3NH2) solution and 50. mL of 2.0 M methylamine hydrochloride
(CH3NH3Cl) solution. The Kb for methylamine is 4.4 x 10-4. What is
the pH of the resulting solution after adding 100 mL of 1.0 M KOH
to the original buffer solution?
The following buffer was prepared: 50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of...
The following buffer was prepared: 50. mL 2.0 M methylamine
(CH3NH2) solution and 50. mL of 2.0 M methylamine hydrochloride
(CH3NH3Cl) solution. The Kb for methylamine is 4.4 x 10-4
What is the pH of the resulting solution after adding 100mL of
1.0M HCl to the original buffer solution?
A) 11.12 B) 10.64 C) 12.32 D) 0.48 E) 5.32 (Correct Answer:
5.32) Please show work, and explain why.
A solution consists of 35 ppm of benzene. The density of the solution is 1.00g/mL. How...
A solution consists of 35 ppm of benzene. The density of the
solution is 1.00g/mL. How many grams of benzene are in 1 g of
solution? How many grams of benzene are in 1.0 L of the solution?
What is the mass percentage of benzene in the solution? Please show
calculations!
What is the pH of the solution which results from mixing 35 mL of 0.50 M...
What is the pH of the solution which results from mixing 35 mL
of 0.50 M NH3(aq) and 35 mL of 0.50 HCI(aq) at 25 degree C? (Kb for
NH3 = 1.8*10^-5). Please show all work. The answer is pH=4.32
2.) Describe and show your calculations how you will make a 50 mL solution of an...
2.) Describe and show your calculations how you will make a 50
mL solution of an ammonia buffer where pH = 10.07 and [NH3] +
[NH4+] = [NH4]T = 10.2 M using concentrated ammonia (28.0% by
weight) and ammonium chloride.
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