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Mashcka [7]
2 years ago
13

"In carrying out a titration of a hydrochloric acid solution with a standard sodium hydroxide solution, a student went beyond th

e end point before reading the volume on the burette. That is, the volume used was larger than the volume required to reach the end point. How will this error affect the calculated concentration of the hydrochloric acid?"
Chemistry
1 answer:
poizon [28]2 years ago
5 0

Answer:

The calculated concentration of HCl will be less than actual.

Explanation:

Suppose during titration, the <em>HCl</em> was taken in burette and the <em>NaOH</em> in the volumetric flask.

Now we will use equivalence formula for the calculation of concentration of HCl.

             N_{1} V_{1} = N_{2} V_{2}

Where L.H.S is for hydrochloric acid and R.H.S is for sodium hydroxide. The terms N and V represent normality and volume respectively.

If we calculate for

                              N_{1} = \frac{N_{2}V_{2} }{V_{1} }

We see that if the volume of the HCl is greater then the concentration of the HCl will be reduced.

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Equation is as follow,

<span>                          4 Na (s)  +  O</span>₂ <span>(g)    →    2Na</span>₂<span>O (s)

According to equation,

      91.92 g (4 moles) of Na produces  =  123.92 g (2 moles) of Na</span>₂O
So,
                    17.4 g of Na will produce  =  X g of Na₂O

Solving for X,
                                   X  =  (17.4 g × 123.92 g) ÷ 91.92 g

                                   X  =  23.45 g of Na₂O
7 0
3 years ago
What increases OH ions​
hram777 [196]

Answer:

A base.

Explanation:

Basic solutions give OH- ions.

7 0
3 years ago
2. Why can we eliminate the claim you circled?
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7 0
3 years ago
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ObIel WiLll unt COl.. USSMS A certain chemical reaction releases 31.2 kJ/g of heat for each gram of reactant consumed. How can y
aleksandr82 [10.1K]

Answer:

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1,080J.\frac{1kJ}{10^{3}J } =1.080kJ

Then,

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here, the amount of remaining substance is 50%,

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what do you mean by radioactive decay ?

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