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alisha [4.7K]
3 years ago
9

If an instrument has 10 ml td +/- 0.01 ml written on it, the user should ..... question 5 options: record 10 ml in the notebook

after using it. record 10.0 ml in the notebook after using it. record 10.00 ml in the notebook after using it. record 5.00 ml in the notebook after using it.
Chemistry
1 answer:
galina1969 [7]3 years ago
6 0

Answer : The correct option is "record 10.00 ml in the notebook after using it."

Explanation :

If an instrument has "10 mL TD" written on it, that means the instrument is meant To Deliver (TD) 10 mL of volume.

Therefore the option that has 5.00 mL is not correct.

"+/- 0.01 mL" indicates the precision of the instrument. We know that no measurement is 100% accurate and there is always some uncertainty associated with any measurement.

Here, 0.01 indicates the uncertainty in the measurement.

When we have 0.01 mL , that means the instrument can record precisely to the hundredths place.

The more the significant figures, the greater is the accuracy of the measurement.

Therefore when we use an instrument that has "+/- 0.01 mL" written on it, we should record the reading as 10.00 mL  


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Read 2 more answers
If you mix 50mL of 0.1 M TRIS acid with 60 mL of0.2 M<br> TRIS base, what will be the resulting pH?
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<u>Answer:</u> The pH of resulting solution is 8.7

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To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}

  • <u>For TRIS acid:</u>

Molarity of TRIS acid solution = 0.1 M

Volume of solution = 50 mL

Putting values in above equation, we get:

0.1M=\frac{\text{Moles of TRIS acid}\times 1000}{50mL}\\\\\text{Moles of TRIS acid}=0.005mol

  • <u>For TRIS base:</u>

Molarity of TRIS base solution = 0.2 M

Volume of solution = 60 mL

Putting values in above equation, we get:

0.2M=\frac{\text{Moles of TRIS base}\times 1000}{60mL}\\\\\text{Moles of TRIS base}=0.012mol

Volume of solution = 50 + 60 = 110 mL = 0.11 L    (Conversion factor:  1 L = 1000 mL)

  • To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:

pH=pK_a+\log(\frac{[salt]}{[acid]})

pH=pK_a+\log(\frac{[\text{TRIS base}]}{[\text{TRIS acid}]})

We are given:

pK_a = negative logarithm of acid dissociation constant of TRIS acid = 8.3

[\text{TRIS acid}]=\frac{0.005}{0.11}

[\text{TRIS base}]=\frac{0.012}{0.11}

pH = ?

Putting values in above equation, we get:

pH=8.3+\log(\frac{0.012/0.11}{0.005/0.11})\\\\pH=8.7

Hence, the pH of resulting solution is 8.7

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