Calculate the osmolarity of each of the following solutions. a. aqueous 0.10M NaCl solution = 0.20 osmol
b. aqueous 0.30M NaNO3 solution = 0.60 osmol
c. aqueous 0.20M CaBr2 solution = 0.60 osmol
d. aqueous 0.50M glucose (C6H12O6) solution = 0.50 osmol
e. aqueous 0.40M Al(NO3)3 solution = 1.6 osmol
And wears are provided, but calculate please!!!

The alkali metals (group 1) consist of lithium (3), sodium (11), potassium (19), rubidium (37), cesium (55), and francium (87). they are soft, metallic solids with low densities and low melting points. based on the data shown in figure 1, how many valence electrons do alkali metals share?

Answer asap need by wednesday morning explain how a buffer works, using an ethanoic acid/sodium ethanoate system including how the system resists changes in ph upon addition of a small amount of base and upon addition of a small amount of acid respectively. include the following calculations in your i. calculate the ph of a solution made by mixing 25cm3 0.1m ch3cooh and 40cm3 0.1m ch3coo-na+. [ka = 1.74 x 10-5 m] ii. calculate the ph following the addition of a 10cm3 portion of 0.08 m naoh to 500cm3 of this buffer solution. iii. calculate the ph following the addition of a 10cm3 portion of 0.08 m hcl to 200cm3 of the original buffer solution.

Suppose you mix one mole of sulfuric acid (h2so4) with 1 mole of sodium hydroxide(naoh). why does the ph of the solution remain below 7? ( explain so i can get better understanding! )