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kati45 [8]
2 years ago
7

Which of the following is the last step in performing a titration? finding out which pH indicator works determining the concentr

ation of an unknown base finding the number of moles of product produced in a reaction determining the molecular masses of the products in the reaction
Chemistry
2 answers:
Zielflug [23.3K]2 years ago
4 0

Answer:   Determining the concentration of an unknown base

Explanation:   While performing a titration,below mentioned steps are followed in the written order -

a)  Finding out which pH indicator works - this is the important and the initial step

b)  After that , one will determine the molecular masses of the products formed in the reaction.

c)  After  determining the molecular mass, number of moles of the product are calculated in order to reach to the conclusion.

d) Thus the final step would be the determiation of the concentration of the unknown base.

kobusy [5.1K]2 years ago
3 0
Answer - D<span>etermining the concentration of an unknown base
</span>
In any titration procedure, the final step would usually be to determine the concentration of the unknown substance, be it the acid or the base. All the other steps listed in the question above are carried out in order to eventually come to the correct calculation of the concentration.
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3 years ago
What is the ratio of lactic acid (Ka = 1.37x^10-4) to lactate in a solution with pH =4.29
hram777 [196]

Henderson–Hasselbalch equation is given as,

                                         pH  =  pKa  +  log [A⁻] / [HA]   -------- (1)

Solution:

Convert Ka into pKa,

                                         pKa  =  -log Ka

                                         pKa  =  -log 1.37 × 10⁻⁴

                                         pKa  =  3.863

Putting value of pKa and pH in eq.1,

                                         4.29  =  3.863 + log [lactate] / [lactic acid]

Or,

                   log [lactate] / [lactic acid]  =  4.29 - 3.863

                   log [lactate] / [lactic acid]  =  0.427

Taking Anti log,

                             [lactate] / [lactic acid]  =  2.673

Result:

           2.673 M  lactate salt when mixed with 1 M Lactic acid produces a buffer of pH = 4.29.

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3 years ago
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See the answer below

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4 0
3 years ago
If the reaction is at dynamic equilibrium at 500 K, which statement applies to the given chemical system?
Alenkinab [10]

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8 0
3 years ago
Read 2 more answers
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