Answer:
pH → 1.13
Explanation:
Our solution is pure HCl
HCl(aq) + H₂O(l) → H₃O⁺(aq) + Cl⁻(aq)
As a strong acid, it is completely dissociated.
1 mol of HCl, can give 1 mol of H⁺ to the medium. Water does not participate. Let's find out M for the acid.
1st step: We convert the mass from mg to g → 327 mg . 1g /1000mg = 0.327 g
2nd step: We convert the mass(g) to moles: 0.327 g / 36.45 g/mol = 8.97×10⁻³ moles
3rd step: We convert the volume from mL to L → 120mL . 1L /1000 mL = 0.120L
Molarity (mol/L) = 8.97×10⁻³ mol / 0.120L = 0.075M
We propose: HCl(aq) + H₂O(l) → H₃O⁺(aq) + Cl⁻(aq)
0.075M 0.075M
pH = - log [H₃O⁺] → - log 0.075 = 1.13 → pH
Answer:
The limiting reactant is the copper
Explanation:
Moles are the standard unit at which you can compare values, and copper has fewer moles than Silver nitrate, so in a reaction, it would be used up first, leaving Silver nitrate in excess.
First write out the balanced equation. 3Cu+2Ag(NO3)3=2Ag+3Cu(NO3)2
Then convert copper from grams to moles
15 g*1 mol cu/63.54 g= 15/63.54 mol cu
Then use the mole ratio to convert Moles Cu to Moles Ag
15/63.54 moles Cu* 2 moles Ag/3 moles Cu
The final awnser is (15*2)/(63.54*3) moles Ag =0.157 moles Ag. If the question wants the answer in grams, convert from moles Ag to grams Ag.
0.157 moles Ag*107.87 g Ag/ mol Ag=16.98 g Ag
A mole of sodium chloride has mass 58.44 grams. You get that from adding the molar masses of sodium and chlorine, which are listed on the periodic table.
<span>58.44 g/mol * 4.40 mol = 257.1 or ≈ 257 grams with 3 significant figures</span>
Take a hypothetical sample of exactly 100 grams of the solution.
(16g urea) / (60.06 g urea/mol) = 0.2664 mol urea
((100 g total) - (16g urea)) = 84.0 g H2O = 0.0840 kg H2O
(0.2664 mol) /0.0840 (kg) = 3.17143mol/kg = 3.18m urea