"how would you make 100 ml of a carbonic acid buffer at 0.5 m and ph = 6.0 using 1.0 m nahco3 and either 1.0 m naoh or 1.0 m hcl and water? "

You first  start by weighing a quatity of NaHCO3 which is by calculating the molecular mass of the salt and then multiply it with the molarity given which is 0.5 M, the gram/mol gotten is then dissolve in some water, add 0.1M NaOH dropwise until the pH is 9.8. Transfer quantitatively to a 100 mL volumetric flask and dilute to the mark. Mix thoroughtly.

Explanation:

molar mass of Na HCO3= 84.01

molarity given= 0.5 M

to get the g/mol to dissolve in 1000 mL , 0.5 x 84.01 =42.005 g/mol=1 L

to get 100 mL , 42.002 divide by 10

=4.2005g/mol

it should have an internal chamber and two thermometers sticking out of the top. the internal chamber will also be closed off from the outside.

explanation:

two years ago, when picking flowers in the mountains back of yosemite valley, i found a book. it was blotted and storm-beaten; all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however; many of the inner pages were well preserved. and although all were more or less stained and torn, whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today; its granite pages have been torn and blurred by the same storms that wasted the castaway book.

two years ago, when picking flowers in the mountains back of yosemite valley; i found a book. it was blotted and storm-beaten, all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however, many of the inner pages were well preserved. and although all were more or less stained and torn; whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today, its granite pages have been torn and blurred by the same storms that wasted the castaway book.