20.0 ml of 0.06 m hcl (in a flask) is titrated with 0.04 m naoh (in a burette). how many milliliters of naoh needs to be used to reach the equivalence point?
a.0.03 ml
b.20.0 ml
c.20 ml
d.30 ml

2.which of the following would you identify a titration curve that involved a strong acid titrated by a weak base?
a. the ph at the equivalence point is lower than 7.
b. the ph at the equivalence point is higher than 7.
c. the titration curve begins at a higher ph and ends at a lower ph.
d. there is a rapid change in ph near the equivalence point (ph = 7).

There is a rapid change in pH near the equivalence point (pH = 7).

Explanation:

At equivalence point the moles of base used is equal to moles of acid taken.

Let us calculate the moles of acid taken.

Moles = molarity X volume (L)

Given

molarity = 0.06 M

Volume =20.0 mL = 20 X 10⁻³ L

moles of HCl = 0.06 X 20 X 10⁻³= 1.2 X 10⁻³

moles of NaOH required = 1.2 X 10⁻³

Thus volume of NaOH used at equivalence point = 30 mL

2) For pH titration curve (for example strong acid and weak base) we observe a rapid change in pH near equivalence point.

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explanation:

in chemistry, adhesion and cohesion are attractive forces that exist between molecules. they hold the molecules together from each other. they are different in that adhesive force exists between molecules of different substance while cohesive force happens between molecules of same substance.

adhesion between water and glass causes water molecules at the edge of water and glass interface to climb up the wall in a narrow glass tube. this is called capillary action. cohesion is what gives glass its shape and causes water to form a droplet.