Write the balanced chemical equation for the acid-base neutralization reaction t

Question

Write the balanced chemical equation for the acid-base neutralization reaction that occurs between HF and KOH. Consider the titration of 50.00 mL of 0.153 M NaOH using 0.0785 M H_2SO_4. Write the balanced chemical equation for the reaction. How many mL of H_2SO_4 are needed to exactly neutralize the base? What will be the molarity of the ionic compound produced at the equivalence point (i.e., the point at which the base has been exactly neutralized)? For each of the following, state whether the molecule is polar or nonpolar. You must provide work (a Lewis structure will suffice) to justify your answers. SO_2

Explanation / Answer

4) the balanced equation is

HF+ KOH=KF+ H2o

5) a) the balanced chemical equation i

2NaoH+H2So4= Na2So4+H2o

b) M1V1 = M2V2

(0.05L)*(0.153M) = (0.0785M)V2

V2 = 0.0974 L

V2 = 974ml

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