Oh, no! you just spilled 85.00 ml of 1.500 m sulfuric acid on your lab bench and need to clean it up immediately! right next to you there is a small jar labeled "15.00 g sodium bicarbonate". will this be enough sodium bicarbonate to neutralize the spilled sulfuric acid? show your work and state all reasoning!

Explanation:

We will balance equation which describes the reaction between sulfuric acid and sodium bicarbonate: as follows.

Next we will calculate how many moles of are present in 85.00 mL of 1.500 M sulfuric acid.

As,       Molarity =

            1.500 M =

                    n = 0.1275 mol

Now set up and solve a stoichiometric conversion from moles of  to grams of . As, the molar mass of is 84.01 g/mol.

                 = 21.42 g

So unfortunately, 15.00 grams of sodium bicarbonate will "not" be sufficient to completely neutralize the acid. You would need an additional 6.42 grams to complete the task.

i don t now

answer: at room temperature (roughly 20 degrees c), you can dissolve 203.9 grams (or 200 grams) of sugar in 100 ml of water. as water temperature increases, the amount of sugar that will dissolve increases, up to about 500 grams of sugar in 100 ml water at 100 degrees c.

explanation: