Buffer Calculations

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Questions

• How are buffer solutions used?
• How do you calculate buffer capacity?
• How do buffer solutions maintain the pH of blood?
• How do you buffer a solution with a pH of 12?
• Why are buffer solutions used to calibrate pH?
• What is the role of buffer solution in complexometric titrations?
• How you would make 100.0 ml of a 1.00 mol/L buffer solution with a pH of 10.80 to be made using only sodium carbonate, sodium hydrogen carbonate and water? How much sodium carbonate and sodium hydrogen carbonate would you use?
• What is the Henderson-Hasselbalch equation?
• What is an example of a pH buffer calculation problem?
• Why is the bicarbonate buffering system important?
• How can I estimate blood pH?
• What are the "Universal" buffer mixtures?
• What does a buffer do in a solution?
• What are the different types of buffering system in the body?
• How does the dilution factor affect a buffer solution?
• Question #b6a38
• Question #6c230
• Question #3c224
• Question #e6995
• Question #54a99
• Question #bd7ca
• Buffer or no buffer? #"45 mL"# of #"0.60 M"# #"KF"# reacts with #"25 mL"# of #"0.60 M"# #"HClO"_4# to yield #"HF"# and #"KClO"_4#, all aqueous.
• What is the net ionic equation for the reaction between #"HOCl"# and #"OCl"^"-"#? What is the pH of a buffer made by mixing 300 mL of 0.50 mol/L #"HClO"# and 400 mL of 0.50 mol/L #"NaClO"#?
• Question #0a0b2
• Question #8fccb
• Question #6f00a
• Question #7507c
• Question #afc26
• Question #998ab
• Question #b3509
• What is the set of chemical equations that describe the buffering action of phosphate buffered saline (PBS)? Calculate theoretically the pH of phosphate buffered saline.
• Question #aa487
• Question #08b39
• Question #48e56
• Question #dd6ba
• Question #fe671
• Question #a8f69
• Question #7d9eb
• Question #262c6
• Question #05115
• A 1.50 L buffer solution is 0.250 M HF and 0.250 M NaF. What is the pH of the solution after the addition of 0.0500 moles of solid NaOH? Assume no volume change. Ka for HF is 3.5x10^-4
• How would you use the Henderson–Hasselbalch equation to calculate the pH of each a solution that contains 1.40% C2H5NH2 by mass and 1.18% C2H5NH3Br by mass?
• 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)?
• How would you rearrange the Henderson–Hasselbalch equation to find out [a/ha] from pH=pKa + log[a/ha] ?
• How would you use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.120 M in HClO and 0.185 M in KClO?
• A solution contains 0.274 M sodium hypochlorite and 0.146 M hypochlorous acid. What is the pH of the solution?
• A buffer is prepared by mixing #1*mol# of acetic acid with #1*mol# of sodium acetate...what is the concentration of the buffer?
• Question #58f8b
• Question #58460
• Question #a3768
• Question #503ff
• How many moles of sodium hypochlorite should be added to 1L of 0.05M hypochlorous acid to form a buffer solution with pH 9.15ssume no changes of volume occurs when NaOCl salt is added?
• A buffer solution is prepared by mixing 1 mole of HA and 1 mole of NaA into 1 L distilled water. Calculate the change in pH when 2t mL of 0.20 M NaOH is added into 500mL of the buffer?
• A buffer was prepared by adding 20g of acetic acid #CH_3COOH# and 20g sodium acetate to enough water to make a 2.0L solution.Determine the pH and write an equation for reaction when a few drops of #HCl# are added to the buffer?
• A buffer solution is prepared by mixing 1.0 mole of HA and 1.0 mole of NaA into 1.0 L distilled water. Calculate the change in pH when 25.0 mL of 0.20 M NaOH is added into 500 mL of the buffer? Given Ka(HA) is 1.75×10^(-5) M
• Question #70577
• A solution P contains 0.55 mol/L ammonia and 0.10 mol/L ammonium chloride. What is the pH of the solution after the addition of 1.0 mL of 0.10 mol/L NaOH?
• What is the pH of a buffer that was prepared by adding 3.96 g of sodium benzoate, #NaC_7H_5O_2#, to 1.00 L of 0.0100 M benzoic acid, #HC_7H_5O_2#?
• Question #545aa
• Question #0365a
• Question #b17d5
• What is the pH of a buffer that consists of 0.100 M #HCOOH# and 0.540 M #HCOONa#?
• If a buffer solution is 0.290 M in a weak base (#K_b = 6.4 xx 10^(-5)#) and 0.520 M in its conjugate acid, what is the pH?
• A student is asked to prepare a buffer solution with pH = 8.6, using one of the following weak acids: HA (#Ka = 2.7 × 10^-3#), HB (#Ka = 4.4 × 10^-6#) or HC (#Ka = 2.6 × 10^-9#). Which acid should she choose?
• A buffer solution is 1.30 M in #NH_3# and 1.20 M in #NH_4Cl#. If 0.120 moles of #NaOH# are added to 1.00 L of the buffer, what is its pH? Assume the volume remains constant. Kb of #NH_3 = 1.8 xx 10^(-5)#.
• You need to produce a buffer solution that has a pH of 5.12. You already have a solution that contains 10 mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution?
• You need to produce a buffer solution that has pH 5.06. You already have a solution that contains 10 mmols of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution?
• How do you calculate the change in pH when 3.00 mL of 0.100 M #"HCl"(aq)# is added to 100.0 mL of a buffer solution that is 0.100 M in #"NH"_3(aq)# and 0.100 M in #"NH"_4"Cl"(aq)# ?
• A 1.00 L buffer solution is 0.150 M in #HC_7H_5O_2# and 0.250 M in #LiC_7H_5O_2#. How do you calculate the pH of the solution after the addition of 100.0 mL of 1.00 M #HCl#? The Ka for #HC_7H_5O_2# is #6.5 × 10^–5#.
• Question #f7626
• Question #9da57
• Question #96889
• Question #f5fc3
• Question #15adf
• Question #f0ac6
• Question #76558
• Question #cc892
• The concentration of carbonic acid in normal blood is 0.029 mol/L and the pKa for carbonic acid is 6.1. Using the Henderson-Hasselbach equation, how do you determine the concentration of bicarbonate ion in normal blood sample which is pH 7.40?
• How would you use the Henderson–Hasselbalch equation to calculate the pH of the solution? A solution that is 0.800 % #C_5H_5N# by mass, and 0.990 % #C_5H_5NHCl# by mass
• How would you use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution that is 0.27 M in formic acid (#HCO_2H#) and 0.50 M in sodium formate (HCO_2Na)?
• A beaker with 120mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.1M. A student adds 6.60mL of a 0.300M HCl solution to the beaker. How much will the pH change?
• Question #92142
• Upon dissolution in water, does sodium acetate give a BASIC or an ACIDIC solution?
• Is it okay to have a #"pH"# above #14#?? Apparently #"1.05 M"# #"NaOH"# has a #"pH"# above #14# at #25^@ "C"#.
• How do you calculate the pH of a buffer?
• How do you solve chemistry buffer problems?
• What #"CH"_3"COO"^(-)# concentration is required to prepare a buffer solution with a pH of 5.10 if #["CH"_3"COOH"]# is 0.150 M? #K_a# of #"CH"_3"COOH"# is #1.8 xx 10^-5#?
• How many milliters of 1.00 M #NaOH# would you have to add to 200ml of 0.150M #HNO_2# to make a buffer with a pH of 4.00?
• Question #2d0ea
• What mass of sodium benzoate should be added to 140.0 mL of a 0.15 M benzoic acid solution to obtain a buffer with a pH of 4.25?
• How would you calculate the pH of the #"0.39 M"# #"NH"_3# #"/"# #"0.73 M"# #"NH"_4"Cl"# buffer system?
• Question #eab13
• You are asked to make a buffer solution with a pH of 2.0. Use the information below to identify an appropriate choice of an acid and a conjugate base to make the buffer?
• How many moles of sodium hypobromite (NaBrO) must be added to a 2.00 L solution of 0.025 M hypobromous acid (HBrO) to form a buffer solution of pH 9.0 (Ka HBrO is 2.5x10^-9)? Assume the volume of solution does not change on addition of NaBrO?
• Question #f3e75
• A buffer is made by dissolving #"NaClO"# and #"HClO"# in water. How do you write equations to show how this buffer neutralizes added H+ and OH-?
• Question #02c04
• Question #45fc9
• Question #a643f
• Question #5252b
• Question #c1b5b
• Question #ff1ed
• Question #af0cd
• 200 ml of 0.1 M sodium hydroxide is mixed with 100 ml of 0.2 M ethanoic acid. What is the pH of the resulting solution?
• What is a buffer?
• Question #bf279
• A solution is made by mixing 500mL of .3M benzoic acid and 400mL of .25M benzoate. What will the pH of the solution be?. Specifically, how do I find the concentration of the acid and base to use in the equation #pH=pKa +log( ([A^(-)])/([HA]))# ?
• Question #4c6d6
• Question #469ae
• Calculate #pH# of buffer solution with #0.1# #M# each of #CH_3COOH# & #CH_3COONa#. What will be the change in #pH# on addition of the following: ? (#pK_a# = #1.8 xx 10^-5#). The total volume of solution is #1# #L#.
• Triethanolamine is a base. What proportion of a 0.04 M solution of this base should be mixed with 0.06 M hydrochloric acid to give 1 litre of buffer solution of pH 7.2 ?
• Which of the following mixtures will form a buffer solution?
• How much ammonium chloride do we need to add to a #20*mL# volume of #NH_3(aq)# at #0.50*mol*L^-1# concentration, to maintain a #pH=9.0#?
• Question #97ac9
• A given volume of a buffer solution contains #6.85 x 10^-3# mol of the weak acid HY and #2.98 x 10^-3# mol of the salt NaY. The pH of the buffer solution is 3.78. How do you calculate the value of #pKa# for the acid HY at this temperature?
• Question #6d2c6
• What is the #pH# of a buffer solution prepared from #50*mL# of sodium hydroxide solution that is #0.220*mol*L^-1# with respect to #NaOH#, and #100*mL# of acetic acid solution that is #0.150*mol*L^-1# with respect to #HOAc#?
• Question #dbab5
• How many millimoles of strong acid or strong base can be added to the solution before any significant change in pH occurs?
• What is the pH of 0.05 mol/L acetic acid? What are the hydronium ion and acetate ion concentrations in a 0.05 mol/L pH 4 acetate buffer?
• Suppose you have #"500.0 mL"# of #"0.200 M"# acetic acid (#K_a = 1.8 xx 10^(-5)#). To make a #"pH"# #4.50# buffer, how many #"mL"# of #"3.0 M"# #"NaOH"# must be added?
• A beaker with #1.50 xx 10^2"mL"# of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.00 mL of a 0.360 M HCl solution to the beaker?
• Question #c18bc
• Why, when an ammonia solution is titrated with a strong acid, the #pH# remains relatively constant up to the addition of a stoichiometric quantity of the acid?
• An #0.500*L# volume of ammonia/ammonium buffer has #pH=9.15#. If #[NH_3]=0.10*mol*L^-1#, what MASS of ammonium chloride does this buffer contain?
• Question #109c2
• Question #00924
• Question #35ef6
• Question #156ba
• Given #250*mL# of #0.200*mol*L^-1# aqueous ammonia, how much ammonium chloride would be added to achieve a #pH-=8.90#?
• Question #f3c37
• Question #7f273
• Question #fc66b
• 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 565 mL of 0.250 M weak acid (Ka = 2.92 × 10-5). What is the pH of the resulting buffer?
• Question #bf42d
• Question #75541
• How do we calculate the #pH# of a buffer that is composed of #HPO_4^(2-)# and #H_2PO_4^(-)#?
• Question #97e59
• Question #12b86
• Question #b7389
• How do I calculate the #"pH"# of the buffer solution when #1.00# #"g"# of potassium ethanoate is dissolved in #50.0# #"cm"^3# of #0.20# #"mol"# #"dm"^-3# ethanoic acid (#"K"_"a"=1.74xx10^-5# #"mol"# #"dm"^-3#)?
• How do I calculate the #"pH"# of the buffer solution formed when #10.0# #"cm"^3# of #0.80# #"mol"# #"dm"^-3# sodium hydroxide is mixed with #50.0# #"cm"^3# of #0.50# #"mol"# #"dm"^-3# ethanoic acid (#"K"_"a"=1.74xx10^-5# #"mol"# #"dm"^-3#)?
• Question #75de2
• Question #26dfc
• Question #dc4c4
• Question #94905
• Question #bf38f
• Question #816f3
• Question #d50ce
• How would you prepare 500 mL of a 0.01 mol/L buffer with pH 7.00 from 0.2 mol/L stock solutions of sodium dihydrogen phosphate and disodium hydrogen phosphate?
• Question #9732f
• Question #a4e04
• What is the pH of a solution of 750.0 mL of 0.500 M #HNO_2# to which 25.00 grams of sodium nitrite has been added (assume no volume change)?
• Question #20193
• Question #a4463
• A buffer solution was prepared from #0.615*L# of weak acid #HA# at #0.250*mol*L^-1# concentration, and a #0.500*L# volume of #NaOH# at #0.130*mol*L^-1# concentration. What is the resultant #pH# of this buffer?
• If the ratio of weak base to conjugate acid is #10:1#, to what extent does the #"pH"# change and does it increase or decrease?
• What is the #pH# of a buffer composed of #0.145*mol*L^-1# #NaNO_2# and #0.125*mol*L^-1# #HNO_2#? How does the #pH# evolve if #2.75*g# of #HCl#, and we ignore any volume change?
• A buffer solution of #NH_3# and #NH_4Cl# has a #pH = 9.26#. If in 100mL of buffer solution, 100 mL of distilled water is added what is the change of #pH#?
• If a buffer contains #"0.110 M"# weak base and #"0.440 M"# of the weak conjugate acid, what is the #"pH"#? The #"pK"_b# is #4.96#.
• Question #7bd01
• Question #b2a5b
• Question #4d24c
• Question #001e7
• Question #2627e
• Given the following molar absorptivities of amino acids in #"0.1 M"# phosphate buffer at #"pH 7"#, find the ratio of the absorbance at #"260 nm"# over #"280 nm"#, the #A260:A280# ratio, for a mixture of #"2 mol"# of #"Trp"# and #"1 mol"# of #"Tyr"#?
• What is the pH of the solution formed by mixing 100 mL of 0.5 mol/L ammonia with 50 mL of 1 M hydrochloric acid?
• Question #ef831
• Question #b75b4
• Question #20274
• How many gm of solid NaOH must be added to 100ml of a buffer solution which is 0.1M each w.r.t acid HA and salt NaA to make the pH of solution 5.5. Given #pK_a#(HA) = 5 (Use antilog (0.5) = 3.16?
• Question #becd4
• What is the pH of a solution made of 0.1 M acetic acid and 0.1 M potassium acetate to which 0.001 mol of KOH has been added?
• A buffer solution was prepared by mixing #"392 mL"# of #"0.301 M"# #"NaClO"# and #"181 mL"# of #"0.281 M"# #"HClO"#. Calculate the #"pH"# of the solution?
• Calculate the #"pH"# change in a buffer solution upon the addition of strong acids / base of known concentration?
• A #"25.0-mL"# sample of #"0.150-mol L"^(-1)# hydrofluoric acid is titrated with a #"0.150-mol L"^(-1)# #"NaOH"# solution. What is the #"pH"# after #"26.0 mL"# of base is added?
• You have a #"250.0-mL"# sample of #"1.00-M"# acetic acid. Assuming no volume change, how much #"NaOH"# must be added to make the best buffer? Calculate the #"pH"# of the best buffer.