Enter the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate.
2 answers:
The net ionic equation: Ag⁺ (aq) + Cl⁻(aq) -> AgCl (s)
<h3>Further explanation </h3>The electrolyte in the solution produces ions.
The equation of a chemical reaction can be expressed in the equation of the ions
For strong electrolytes (the ionization rate = 1) is written in the form of separate ions, while the weak electrolyte (degree of ionization <1) is still written as an un-ionized molecule
In the ion equation, there is an ion spectator that is the ion which does not react because it is present before and after the reaction
When these ions are removed, the ionic equation is called the net ionic equation
For gases and solids including water (H₂O) can be written as an ionized molecule
So only the dissolved compound is ionized ((expressed in symbol aq)
Formation of precipitating compounds that cause reactions can occur from double-replacement reactions
Solubility Rules:
- 1. soluble compound
All compounds of Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺, and NH₄⁺
All compounds of NO₃⁻ and C₂H₃O₂⁻
Compounds of Cl⁻, Br⁻, I⁻ except Ag⁺, Hg₂²⁺, Pb²⁺
Compounds of SO₄²⁻ except Hg₂²⁺, Pb²⁺, Sr²⁺, Ba²⁺
- 2. insoluble compounds
Compounds of CO₃²⁻ and PO₄³⁻ except for Compounds of Li +, Na +, K +, Rb +, Cs +, and NH₄ +
Compounds of OH− except Compounds of Li +, Na +, K +, Rb +, Cs +, NH₄⁺, Sr²⁺, and Ba²⁺
The reaction between AgNO₃ (aq) and NaCl (aq)
AgNO₃ (aq) + NaCl (aq) ⇒AgCl (s) + NaNO₃ (aq)
AgCl is an insoluble compound, so reactions can take place and double-replacement reactions occur
Complete ion reaction:
the net ionic equation
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The question is incomplete, here is the complete question:
If 65 mL of sulfuric acid and 25 mL of sodium hydroxide were mixed and the solution had a density of 1.01 g/mL, What is the heat of the calorimeter in kJ given the temperature change of the above equation is -5.5 K. You may assume the solution has a heat capacity of 4.180 J/gK. Express your final answer in kJ and with 2 decimal places
<u>Answer:</u> The heat of the calorimeter is 2.09 kJ
<u>Explanation:</u>
To calculate the mass of solution, we use the equation:
Density of solution = 1.01 g/mL
Volume of solution = [65 + 25] mL = 90 mL
Putting values in above equation, we get:
To calculate the heat released by the reaction, we use the equation:
where,
q = heat released
m = mass of solution = 90.9 g
c = heat capacity of solution = 4.180 J/g.K
= change in temperature = -5.5 K
Putting values in above equation, we get:
Heat released by the solution will be equal to the heat absorbed by the calorimeter.
<u>Sign convention of heat:</u>
When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.
Heat absorbed by the calorimeter = -(-2.09) = 2.09 kJ
Hence, the heat of the calorimeter is 2.09 kJ