✔ 最佳答案
1.
A: no. of mole = volume x molarity = (10/1000) x 3 = 0.03 mole
mass = molar mass x no. of mole = (23+16+1) x 0.03 = 1.2 g
B: no. of mole = 0.04 mole
mass = 1.6 g
C: mass = volume x concentration = (80/1000) x 6 = 0.48 g
D: mass = (100/1000) x 8 = 0.8 g
2.
first write the dissociation equations:
Na3PO4 ------> 3Na(+) + PO4(3-) one mole of salt gives 4 mole of ions
K2SO4 ------> 2K(+) + SO4(2-) one mole of salt gives 3 moles of ions
KNO3 ------> K(+) + NO3(-) one mole of salt gives 2 moles of ions
AgNO3 ------> Ag(+) + NO3(-) one mole of salt gives 2 moles of ions
A: conc. of salt = molarity x volume = 0.1 x (60/1000) = 0.006 mole
no of mole of ions = 0.006 x 4 = 0.024 mole
B: conc. = 0.006 mole
ion = 0.018 mole
C: conc. = 0.05 x (90/1000) = 0.0045 mole
ion = 0.0090 mole
D: conc. = 0.006 mole
ion = 0.0120 mole
3.
similar to question 2.
first write down the acid ionization / salt dissociation equations;
then calculate no. of mole of ions given per mole of acid;
finally calculate the concentration of salt and ions.
4.
B, C and D are in fact talking about same thing. so neither one could be the answer ----
D: same mass (106g) of sodium carbonate is added into total volume of 1000cm3 of water, so it's same as C.
B: both mass and total volume of water (106g --> 10.6g, 1000cm3 --> 100cm3) are reduced to one-tenth, so concentration remains the same.
nonetheless, i'll include the method of calculation of concentration.
A: mass = 10.6 g
no. of mole = 10.6 / (23x2 + 12 + 16x3) = 0.1 mole
volume of water = 10cm3 = 0.001dm3
thus molarity = n. of mole / volume = 0.1 / 0.001 = 10 M