Answer is: 53 milliliters of KOH are required.
Balanced chemical reaction:
2KOH(aq) + H₂SO₄(aq) → 2H₂O(l) + K₂SO₄(aq).
N(KOH) = 0.0050 N; normality of potassium hydroxide solution.
V(H₂SO₄) = 53 mL; volume of sulfuric acid.
N(H₂SO₄) = 0.0050 N; normality of sulfuric acid.
Na·Va = Nb·Vb.
0.0050 N · 53 mL = 0.0050 N · V(KOH).
V(KOH) = 53 mL; volume of potassium hydroxide solution.
OK so basically you want to control the experiment because you want to make sure that the data to be valid.
Answer:
Divide 6 grams by the atomic mass of fluorine.
Explanation:
Number of moles = Mass / atomic mass of fluorine
Given data:
Mass of fluorine = 6 g
How to convert into moles of fluorine = ?
Solution:
Number of moles = Mass / atomic mass of fluorine
Number of moles = 6 g/ 19 g/mol
Number of moles = 0.32 mol
So in order to convert the 6 g of fluorine into moles we have to divide the 6 by atomic mass of fluorine.
Answer:
[KCl] = 1.2 M
Explanation:
We need to complete the reaction:
2KCl(aq) + Pb(NO₃)₂(aq) → 2KNO₃(aq) + PbCl₂(s)↓
By stoichiomety we know that 1 mol of chloride needs 1 mol of nitrate to react:
Let's find out the moles of nitrate, we have:
Molarity = mol/volume(L)
We convert the volume → 30 mL . 1L/1000mL = 0.030L
Molarity . volume(L) = moles → 0.400 M . 0.030L = 0.012 moles
Therefore, we can make a rule of three.
1 mol of nitrate reacts with 2 moles of chloride
Then, 0.012 moles of nitrate must react with (0.012 . 2) / 1 = 0.024 moles of KCl
We convert the volume from mL to L → 20 mL . 1L /1000mL = 0.020L
Molarity = mol /volume(L) → 0.024 mol /0.020L = 1.2 M
