Questions: PRELABORATORY ASSIGNMENT 1. Write the complete equations for the reactions that would occur if the following pairs of solutions were mixed. Be sure to indicate the state of reaction products. You can refer to table 6 in lab manual or the solubility rules in our textbook to find out the solubility of the products. (1) BaCl2(aq) + KIO3(aq) → (2) Sr(NO3)2(aq) + Na2 SO4(aq) → (3) Pb(NO3)2(aq) + NaOH(aq) → (4) CuSO4(aq) + Na2 C2 O4(aq) →

PRELABORATORY ASSIGNMENT 1. Write the complete equations for the reactions that would occur if the following pairs of solutions were mixed. Be sure to indicate the state of reaction products. You can refer to table 6 in lab manual or the solubility rules in our textbook to find out the solubility of the products. (1) BaCl2(aq) + KIO3(aq) → (2) Sr(NO3)2(aq) + Na2 SO4(aq) → (3) Pb(NO3)2(aq) + NaOH(aq) → (4) CuSO4(aq) + Na2 C2 O4(aq) →
Transcript text: PRELABORATORY ASSIGNMENT 1. Write the complete equations for the reactions that would occur if the following pairs of solutions were mixed. Be sure to indicate the state of reaction products. You can refer to table 6 in lab manual or the solubility rules in our textbook to find out the solubility of the products. (1) $\mathrm{BaCl}_{2}(\mathrm{aq})+\mathrm{KIO}_{3}(\mathrm{aq}) \rightarrow$ (2) $\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow$ (3) $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq}) \rightarrow$ (4) $\mathrm{CuSO}_{4}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(\mathrm{aq}) \rightarrow$
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Solution

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Solution Steps

Step 1: Write the complete equation for the reaction between $\mathrm{BaCl}_{2}(\mathrm{aq})$ and $\mathrm{KIO}_{3}(\mathrm{aq})$

When $\mathrm{BaCl}_{2}(\mathrm{aq})$ and $\mathrm{KIO}_{3}(\mathrm{aq})$ are mixed, the possible products are $\mathrm{Ba(IO}_{3})_{2}$ and $\mathrm{KCl}$. According to solubility rules, $\mathrm{Ba(IO}_{3})_{2}$ is insoluble in water and will precipitate out, while $\mathrm{KCl}$ is soluble.

\[ \mathrm{BaCl}_{2}(\mathrm{aq}) + 2\mathrm{KIO}_{3}(\mathrm{aq}) \rightarrow \mathrm{Ba(IO}_{3})_{2}(\mathrm{s}) + 2\mathrm{KCl}(\mathrm{aq}) \]

Step 2: Write the complete equation for the reaction between $\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ and $\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})$

When $\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ and $\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})$ are mixed, the possible products are $\mathrm{SrSO}_{4}$ and $\mathrm{NaNO}_{3}$. According to solubility rules, $\mathrm{SrSO}_{4}$ is insoluble in water and will precipitate out, while $\mathrm{NaNO}_{3}$ is soluble.

\[ \mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) + \mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{SrSO}_{4}(\mathrm{s}) + 2\mathrm{NaNO}_{3}(\mathrm{aq}) \]

Step 3: Write the complete equation for the reaction between $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ and $\mathrm{NaOH}(\mathrm{aq})$

When $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ and $\mathrm{NaOH}(\mathrm{aq})$ are mixed, the possible products are $\mathrm{Pb(OH)}_{2}$ and $\mathrm{NaNO}_{3}$. According to solubility rules, $\mathrm{Pb(OH)}_{2}$ is insoluble in water and will precipitate out, while $\mathrm{NaNO}_{3}$ is soluble.

\[ \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) + 2\mathrm{NaOH}(\mathrm{aq}) \rightarrow \mathrm{Pb(OH)}_{2}(\mathrm{s}) + 2\mathrm{NaNO}_{3}(\mathrm{aq}) \]

Final Answer

  1. \(\mathrm{BaCl}_{2}(\mathrm{aq}) + 2\mathrm{KIO}_{3}(\mathrm{aq}) \rightarrow \mathrm{Ba(IO}_{3})_{2}(\mathrm{s}) + 2\mathrm{KCl}(\mathrm{aq})\)
  2. \(\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) + \mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{SrSO}_{4}(\mathrm{s}) + 2\mathrm{NaNO}_{3}(\mathrm{aq})\)
  3. \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) + 2\mathrm{NaOH}(\mathrm{aq}) \rightarrow \mathrm{Pb(OH)}_{2}(\mathrm{s}) + 2\mathrm{NaNO}_{3}(\mathrm{aq})\)
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