Topic
Q:
\( C _ { 2 } H _ { 6 } + O _ { 2 } \rightarrow CO _ { 2 } + H _ { 2 } O \)
Q:
How many formula units of ammonium phosphate are
Needed to make 100.00 grams of ammonium phosphate?
Q:
The pH of a fruit juice is 2.8. Find the hydronium ion concentration, \( \left[\mathrm{H}_{3} \mathrm{O}^{+}\right] \), of the juice. Use the formula \( \mathrm{pH}=-\log \left[\mathrm{H}_{3} \mathrm{O}^{+}\right] \).
The hydronium ion concentration \( \left[\mathrm{H}_{3} \mathrm{O}^{+}\right] \)is approximately \( \square \) moles per liter.
(Use scientific notation. Use the multiplication symbol in the math palette as needed. Round to the nearest tenth as needed.)
Q:
Question 1
Which, if any, of the substances had resonance structures? How many resonance structures did each substance have?
\( \begin{array}{lllll}\text { B } \quad \mid \quad \underline{\cup} \quad \vdots & \vdots & T^{2} & T_{2}\end{array} \)
Q:
1. Reúnanse en paréas para resolver los siguie
a. \( \mathrm{CaF}_{2}+\mathrm{H}, \mathrm{SO}, \mathrm{CaSO}+\mathrm{HF} \)
Q:
Answer the questions on the space provided on the question paper next to the question. Show your
working outs wherever necessary.
Q1. If the concentration of chromate ions \( \left(\mathrm{CrO}_{4}^{2}\right) \) is \( 6.30 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \) a: the point when the \( \mathrm{Ag}_{2} \mathrm{CrO}_{4} \)
starts to precipitate, calculate the concentration of \( \mathrm{Ag}^{+} \)ions in the solution in the \( \mathrm{K}_{s p} \) of is \( \mathrm{Ag}_{2} \mathrm{CrO}_{4} \) is \( 1.3 \times \)
\( 10^{-12} \)
The equilibrium is:
The \( \mathrm{K}_{s p} \) expression is:
Q:
2. Los ácidos hidrácidos no contienen
oxígeno. Son ácidos binarios (contienen dos
elementos) formados por la combinación del
hidrógeno con un no metal. Un ejemplo es el
HI cuyo nombre es
\( \begin{array}{ll}\text { A. Acido yodhídrico } & \text { B. Acido yódico } \\ \text { C. Acido yodoso } & \text { D. Acido periódico }\end{array} \)
Q:
1. El óxido formado cuando el hierro utiliza
su menor número de oxidación (+2) se
denomina óxido ferroso y si utiliza el mayor
número de oxidación ( +3 ) se denomina
óxido férrico. Si el menor número de
oxidación del Fe es (+2) y el oxígeno trabaja
con \( (-2) \) entonces la fórmula para el óxido
ferroso es
\( \begin{array}{ll}\text { A. } \mathrm{FeO} & \text { B. FeO } \\ \text { C. } \mathrm{Fe}_{2} \mathrm{O}_{3} & \text { D. } \mathrm{Fe} \mathrm{O}\end{array} \)
Q:
Indicate the most likely ion that each of the following will form.
(a) Ba
(b) In
(c) S
(d) Br
(e) N
Q:
Solve the ideal gas equation for the variable \( (1 / V) \). That means fill in the rest of the equation.
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