A student is performing a titration to determine the concentration of a 20.0 mL sample of hydrochloric acid. What did the studen
1 answer:
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Explanation:
Moles of compound =
We have ;
Volume of solution = 600 mL = 0.600 L ( 1 mL = 0.001 L)
Moles of NaOH = n
Molarity of the solution = 3 M
n = 3 M × 0.600 L = 1.800 mol
Mass of 1.800 mole sof NaOH :
1.800 mol × 40 g/mol = 72.0 g
Preparation:
Weight 72.0 grams of sodium hydroxide and add it to the 500 mL of volumetric flask along with some water. Dissolve the all the solute by adding small proportion of water. After the solution becomes clear make the water upto the mark of 500 ml.
Transfer the solution to a bigger beaker and 100 mL of water more to it.
Answer:
1) Favor formation of reactant
2) Favor formation of product
3) Favor formation of product
4) Favor formation of product
5) Favor formation of product
Explanation:
The reaction is
The reaction is endothermic
1. Adding hydrobromic acid (HBr)
It will increase the amount of bromide ion. Bromide ion is one of the product so it will favor formation of reactant.
2. Lowering the concentration of bromide (Br-) ions
As we are decreasing the the concentration of product it will favor formation of more products
3. Heating the concentrations
If we are heating the mixture, it will increase the temperature and it will favor endothermic reaction. Thus will favor formation of product.
4. Adding solid silver bromide (AgBr)
If we are adding silver bromide it means we are increasing the concentration of reactant, it will favor formation of products
5. Removing silver (Ag+) ions
Removing silver ions means we are decreasing the concentration of product thus it will favor formation of products.