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how can i calculate the ph of a stock acetic acid solution given the following: pKa of acetic acid=4.75, concentration of acetic acid = 1.1009M. then, how can i calculate the ph of a stock sodium acetate solution given the following: concentration of sodi...

question regarding equivalence point and end point calculations: how can i calculate the concentration of an unknown using a graph of ph values of a solution and ml of hcl? from the graph, i know that the equivalence point is 11 ml at ph 2.32. similarly,...

how can i calculate the volume of 3 M HCl needed to change the ph of 75 ml of undiluted buffer by one ph unit (buffer capacity). i know that pka is 4.75, acetic acid is 1.1009 M for 100 ml, and sodium acetate is 1.0113 M for 100ml. i have calculated the m...

please let me know if i should provide any other information

im still not sure how to get Kb. so for ka i did 10^-4.75 and got 1.78x10^-5. then using the ice table and the 1.1009 for HA, i got x=4.4x10^-3. then to get the ph, i did -log(x) = 2.35. do i use the same ka of 1.78x10^-5 for kb?

25 mL of 0.09607 M ammonia was titrated with unknown hydrochloric acid

:/ you guys deleted my post and i was just asking for help

got it, thank you!

no worries i am not in a rush, thanks for your help

100 ml of acetic acid and 100ml of sodium acetate were mixed (which is the buffer solution). then hcl (3 M) was added to 75 ml of the buffer solution

what i did was calculate the moles of the acid and acetate: acetic acid: n=(1.1009 x .1L x .075L) / .2L =0.04 did the same for sodium acetate: n=0.03 then 3.75=4.75+log (0.03-x)/(0.04+x) x= moles of HCl then to calculate volume of hcl = moles of hcl/3M no...