Ionic formulas of reactants as they actually exist in solution ionic formulas of

Question

Ionic formulas of reactants as they actually exist in solution ionic formulas of products as they actually exist in solution: Complete ionic equation (be sure to specify nature of all materials) Appearance of reactants (description of each matenal BEFORE mixing Write the possible molecular equation: Observation after mixing:(Evidence of reaction) Ionic formulas of reactants as they actually exist in solution. Ionic formulas of products as they actually exist in solution: Complete ionic equation (be sure to specify nature of all matenals):

Explanation / Answer

b. I believe you are looking for answers to part b.

1. Since both HCl and NaOH are clear, colourless solutions, we use an acid-base indicator to determine the presence of the excess acid or the base in the solution. Phenolpthalein is a good acid-base indicator. Since you have not mentioned which indicator was used, I will tell you the colour of HCl (aq) after phenolphthalein addition. The colour is pale to colourless. Another good indicator for this titration is methyl orange, which has a red colour in HCl medium (when no NaOH is added).

2. The molecular equation is

HCl + NaOH -------> NaCl + H2O

3. I will assume that we are using phenolphthalein indicator. In acidic medium, the indicator is colourless. Once we start adding NaOH from the burette, there is a faint pink colour which is quickly discharged. The colour gets intense as more and more NaOH is added, but the pink colour is quickly discharged in acid medium. Finally, once the end point is reached and we add an excess of NaOH (just one drop extra is sufficient), the solution shows a deep pink colour and this colour is permanent.

4. In aqueous medium, HCl, being a strong acid, exists as ions.

HCl (aq) --------> H+ (aq) + Cl- (aq).

Simialrly, NaOH is a strong base and exists as ions in aqueous solution.

NaOH (aq) -------> Na+ (aq) + OH- (aq)

5. In solution, NaCl, which is formed by the reaction between aqueous HCl and NaOH, dissociates into Na+ and Cl-. H2O remains undissociated.

NaCl (aq)-------> Na+ (aq) + Cl- (aq)

6. The complete ionic equation is

H+ (aq) + Cl- (aq) + Na+ (aq) + OH- (aq) ----------> Na+ (aq) + Cl- (aq) + H2O (l)

7. The net ionic equation is simply the exchange of Cl- and Na+.

H+ (aq) + OH- (aq) --------> H2O (l)

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