Calculate the pKa value for the following acids. Nitrous acid (HNO2),
2018年5月10日 · Calculate the pKa value for the following acids. Nitrous acid (HNO2), #K_a = 4.5 xx 10^(-4)#?
How would you find the appropriate buffer with given pKa's
2016年2月14日 · Meanwhile for phosphate buffer, the pKa value of H_2PO_4^- is equal to 7.2 so that the buffer system is suitable for a pH range of 7.2+-1 or from 6.2 to 8.2. Since the target pH of the buffer to be prepared is 5.0, the best buffer system to use will be the acetate buffer since 5.0 fall in the maximum buffering range for this buffer system.
Order in the increasing order of acidity:HCl, H2SO4, HF, HCl
2018年1月10日 · Order in the increasing order of acidity:HCl, H2SO4, HF, HCl, HI, HBr, HNO3, HBrO, HClO, HClO3, HClO4, H2S, H3PO4(?)
Buffer Calculations - Chemistry - Socratic
You need to prepare 100.0mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa=4.20) and 0.240 M sodium benzoate. How much of each solution should be mixed to prepare the buffer? 500.0 mL of 0.140 M NaOH is added to …
How would you use the Henderson-Hasselbalch equation to
2015年11月17日 · How would you use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution that is 0.27 M in formic acid (HCO2H) and 0.50 M in sodium formate (HCO2Na)?
A 1.00 L solution contains 19.52 g of nitrous acid, HNO2 ... - Socratic
2018年5月1日 · A 1.00 L solution contains 19.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.56?
The pH of 0.02 M solution of an unknown weak acid is 3.7
2016年1月21日 · Knowing the pH, you know the concentration of protons: -log["H"^(+)] = "pH" = 3.7 ["H"^(+)] = 10^(-3.7) "M" Now, since the weak (monoprotic) acid dissociates into its conjugate base and a proton, the "mol"s of protons are equimolar with the "mol"s of conjugate base---the protons came FROM the weak acid, so the conjugate base that forms must be equimolar with the protons given out to the solvent.
The pH of a 0.100 M solution of an aqueous weak acid - Socratic
2016年2月13日 · 1.0 * 10^(-7) Start by writing a balanced chemical equation for the partial ionization of the acid "HA"_text((aq]) + "H"_2"O"_text((l]) rightleftharpoons "A"_text((aq])^(-) + "H"_3"O"_text((aq])^(+) Notice that you have 1:1 mole ratios across the board. For every mole of acid that ionizes in aqueous solution, you get one mole of its conjugate base and one mole of hydronium ions, "H"_3"O ...
A 1.00 L buffer solution is 0.150 M in HC_7H_5O_2 and 0.250
2016年4月11日 · You can do it like this: It looks like the acid is benzoic acid C_6H_5COOH For short - hand I'll call this HA Benzoic acid dissociates: HA_((aq))rightleftharpoonsH_((aq))^(+)+A_((aq))^-" "color(red)((1)) The lithium salt provides a large reserve of the co - base A^- by dissociating completely: LiA_((s))rarrLi_((aq))^(+)+A_((aq))^-" "color(red)((2)) The initial no. moles of A^- is given by: nA ...
A 25.0 ml sample of 0.150 M nitrous acid is titrated with a0
2018年4月16日 · When the titration occurrs you have used 25,0 mL of NaOH so you in total have 50.0 mL of #NaNO_2# that (because the volume is double) will be 0.075 M