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makvit [3.9K]
3 years ago
8

Identify the number with the correct number of significant figures for each step of the calculation and for the final answer. No

te that 2 is an exact number. y equals 2.10 StartBracket 9.0 plus 2 times 35.35 EndBracket. 2 (35.35) =
Chemistry
2 answers:
pav-90 [236]3 years ago
8 0

Answer:

70.70

Explanation:

Just got it right on edge

lara [203]3 years ago
7 0

Answer: The answer is 167

Explanation: This is because that was right on edg. so yea heart this tho plsss

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A sample of a gas has volume 78.5ml at 318.15 K.. What Volume at will the sample occupy at 273. 15 K when the pressure is held c
DochEvi [55]

Charles’ Law

V₁/T₁=V₂/T₂

78.5/318.15=V₂/273.15

V₂=67.4 ml

7 0
1 year ago
What is the volume mL of 2 degree celsius?
Anestetic [448]

Answer:

Question not very specific, but here is an answer you might be looking for. Density of object at 2 degrees C, 0.99997 g/mL. Hope it IS the answer you are looking for!

Explanation:

7 0
3 years ago
A student needs to prepare 50.0 mL of a 1.20 M aqueous H2O2 solution. Calculate the volume of 4.9 M H2O2 stock solution that sho
Nonamiya [84]

Answer : The volume of 4.9 M H_2O_2 stock solution used to prepare the solution is, 12.24 ml

Solution : Given,

Molarity of aqueous H_2O_2 solution = 1.20 M = 1.20 mole/L

Volume of aqueous H_2O_2 solution = 50.0 ml = 0.05 L

(1 L = 1000 ml)

Molarity of H_2O_2 stock solution = 4.9 M = 4.9 mole/L

Formula used :

M_1V_1=M_2V_2

where,

M_1 = Molarity of aqueous H_2O_2 solution

M_2 = Molarity of H_2O_2 stock solution

V_1 = Volume of aqueous H_2O_2 solution

V_2 = Volume of H_2O_2 stock solution

Now put all the given values in this formula, we get the volume of H_2O_2 stock solution.

(1.20mole/L)\times (0.05L)=(4.9mole/L)\times V_2

By rearranging the term, we get

V_2=0.01224L=12.24ml

Therefore, the volume of 4.9 M H_2O_2 stock solution used to prepare the solution is, 12.24 ml

3 0
3 years ago
PLEASE HELP FASTTT!!!!
Umnica [9.8K]
I did this when I was younger
4 0
3 years ago
Suppose you are titrating vinegar, which is an acetic acid solution of unknown strength, with a sodium hydroxide solution accord
Marina CMI [18]

Answer:

M_{acid}=0.563M

Explanation:

Hello there!

In this case, given the neutralization of the acetic acid as a weak one with sodium hydroxide as a strong base, we can see how the moles of the both of them are the same at the equivalence point; thus, it is possible to write:

M_{acid}V_{acid}=M_{base}V_{base}

Thus, we solve for the molarity of the acid to obtain:

M_{acid}=\frac{M_{base}V_{base}}{V_{acid}} \\\\ M_{acid}=\frac{33.98mL*0.1656M}{10.0mL}\\\\ M_{acid}=0.563M

Regards!

5 0
3 years ago
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