Answer:
pH = 4.45
Explanation:
We need to find the pH of solution of HCl. We know that, pH of a solution is given by :
Put all the values,
So, the pH of the solution of HCl is 4.45.
1. The molar mass of Fe2(CO3)3 is 291.72 g/mol. This means that 45.6 g is equivalent to 0.156 mol. Dividing by the 0.167 L of water gives a solution of 0.936 M.
2. Multiplying (0.672 M)(0.025 L) = 0.0168 mol. The molar mass of Ni(OH)2 is 92.71 g/mol, so multiplying by 0.0168 mol = 1.56 grams. Therefore you would need to dissolved 1.56 g of Ni(OH)2 into 25 mL of water.
3. Fe2(CO3)3 + Ni(OH)2 --> Fe(OH)3 + NiCO3Balancing: Fe2(CO3)3 + 3Ni(OH)2 --> 2Fe(OH)3 + 3NiCO3The reaction quotient is:[Fe(OH)3]^2 * [NiCO3]^3 / [Fe2(CO3)3][Ni(OH)2]^3= (0.05)^2 * (1.45)^3 / (0.936)(0.672)^3= 0.0268Since this is < 1, it implies that the reactants are favored at equilibrium.
Greetings!
To find the empirical formula you need the relative atomic mass of each element!
C = 12
F = 19
You can simply change the percentages into full grams
C = 13.64g
F = 86.35g
Then you use this to find the Number of moles = amount in grams / atomic mass
C = 13.64 ÷ 12 = 1.13
F = 86.35 ÷ 19 = 4.544
Then divide each number of moles by the smallest value:
C = 1.13 ÷ 1.13 = 1
F = 4.544 ÷ 1.13 = 4.02 ≈ 4
So that means that there are 1 Carbon and 4 Fluorine. This means the empirical formula would be:
CF₄
Hope this helps!
The correct answer to your question is: carbon dioxide.
Answer:
Add more pieces of zinc (2n) to the mixture
Heat the hydrochloric acid (HC) solution.
Explanation:
The reaction rate is simply the speed of the reaction. It is usually monitored by the rate at which the concentration of either of the reactants or products are changing per unit of time.
The factors affecting the rate of reactions are:
- Nature of the reactants
- Concentration or pressure of gases
- Temperature of the reaction
- Availability of catalysts
- Sunlight
In this problem, if the concentration of the zinc increases, the rate of reaction will increase.
If the temperature of HCl increases, so also the rate of the reaction.