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KCO Indicator Colof pH Range Indicated Range Overlap Calculated pH Thymol Blue Blue Metuersel Purple Purple Brompbenol blue Purple Methyl Red Yellow Enter pH range in common for all indicators Enter Calculated pH Bromeresol Green Blue Phenol Red Pink Phenol-phhalien Pink Red Cabbage Green This salt contains Choose an item. Calculate the pH of the 0.10 M solution of this salt using the methods described in the Introduction. Record your answers in the Calc pH column. Related Ka and K. values are listec at the end of this lab. In your lab instructions, show your work for this calculation. Take a phon of your work, include your name and date in the photo and insert the photo below. Enter photo of your work here

KCO Indicator Colof pH Range Indicated Range Overlap Calculated pH Thymol Blue Blue Metuersel Purple Purple Brompbenol blue Purple Methyl Red Yellow Enter pH range in common for all indicators Enter Calculated pH Bromeresol Green Blue Phenol Red Pink Phenol-phhalien Pink Red Cabbage Green This salt contains Choose an item. Calculate the pH of the 0.10 M solution of this salt using the methods described in the Introduction. Record your answers in the Calc pH column. Related Ka and K. values are listec at the end of this lab. In your lab instructions, show your work for this calculation. Take a phon of your work, include your name and date in the photo and insert the photo below. Enter photo of your work here

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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HOC3- = 4.8x10^-11
K.CO Indicator Colot pH Range Indicated Range Overlap Calculated pH Thymol Blue Blue Meturel Purple Purple Brompbenol blue Purple Methyl Red Yellow Enter pl range in common for all indicators Enter Calculated pil Bromerssal Green Blue Phenol Red Pink Phenol-phthalien Pink Red Cabbage Green This salt contains Choose an item. Calculate the pH of the 0.10 M solution of this salt using the methods described in the Introduction. Record your answers in the Calc pH column. Related K. and K, values are listed at the end of this lab. In your lab instructions, show your work for this calculation. Take a photo of your work, include your name and date in the photo and insert the photo below. Enter photo of your work here
Transcribed Image Text:K.CO Indicator Colot pH Range Indicated Range Overlap Calculated pH Thymol Blue Blue Meturel Purple Purple Brompbenol blue Purple Methyl Red Yellow Enter pl range in common for all indicators Enter Calculated pil Bromerssal Green Blue Phenol Red Pink Phenol-phthalien Pink Red Cabbage Green This salt contains Choose an item. Calculate the pH of the 0.10 M solution of this salt using the methods described in the Introduction. Record your answers in the Calc pH column. Related K. and K, values are listed at the end of this lab. In your lab instructions, show your work for this calculation. Take a photo of your work, include your name and date in the photo and insert the photo below. Enter photo of your work here
For a 0.10 M sodium acetate solution, the calculation is as follows. C2H3O2 + HL0 S HC2H302 + OH 0. 0. Initial concentration Change in conc. Equilibrium conc. 0.10 +x +x+ -X 0.10-x KB(C2H3O2) = Kw 10-14 %3D Ka(HCZH302) 18x10-5= 5.56 x 1010 x2 Kb = 5.56 x 10-10 = x [OH]= 7.46 x 10-6 pOH = 5.13; pH = 8.87 0.10-x Some ions are amphiprotic meaning they can potentially act as both an acid or as a base when dissolved in water. They are typically negative jons that also contain acidic hydrogen. They are also conjugate bases of weak polyprotic acids. Some examples of this type of ion are the hydrogen oxalate ion, HC2O4 and the monohydrogen phosphate ion, HPO42. The pH for an amphiprotic ion such as HA can be found using the following equation pH = pKai+ pKa2 where Kal is the first dissociation constant for a diprotic acid, H2A and Ka2 is the second dissociation constant for the conjugate of the diprotic acid, HA". For example, the ion HC2O4 is derived from the diprotic acid H2C2O4. H2C2O4 has first and second dissociation constants of Kal = 5.6x10-² and Ka2 = 5.1x10-5. pKal = 1.25 and pKa2 = 4.29. So to find the pH of a salt solution containing this ion, use the above equation. 1.25+ 4.29 pH = = 2.77 Certain metal ions can also affect the pH of a solution. They do this by first forming a hydrated complex ion. If the metal ion is sufficiently small in size and/or highly positively charged, then a hydrogen ion from one of the water molecules can detach resulting in an acidic solution. For example, Zn2+ forms the complex Zn(H2O)6²+ in aqueous solution. It can then react as follows. Zn(H2O)62+ + H2O S Zn(H2O)5(OH)* + H3O* Ka = 2.5x10-10 The hydronium ion concentration can then be determined using a simple ICE calculation and from there the pH determined. If neither ion in a salt affects the pH, then the solvent water is the only substance that affects the pH and will give a pH = 7. In rare cases, both ions may affect the pH if the cation is the conjugate acid of a weak base AND the anion is the conjugate base of a weak acid. In this case, a general determination of acidic, 18
Transcribed Image Text:For a 0.10 M sodium acetate solution, the calculation is as follows. C2H3O2 + HL0 S HC2H302 + OH 0. 0. Initial concentration Change in conc. Equilibrium conc. 0.10 +x +x+ -X 0.10-x KB(C2H3O2) = Kw 10-14 %3D Ka(HCZH302) 18x10-5= 5.56 x 1010 x2 Kb = 5.56 x 10-10 = x [OH]= 7.46 x 10-6 pOH = 5.13; pH = 8.87 0.10-x Some ions are amphiprotic meaning they can potentially act as both an acid or as a base when dissolved in water. They are typically negative jons that also contain acidic hydrogen. They are also conjugate bases of weak polyprotic acids. Some examples of this type of ion are the hydrogen oxalate ion, HC2O4 and the monohydrogen phosphate ion, HPO42. The pH for an amphiprotic ion such as HA can be found using the following equation pH = pKai+ pKa2 where Kal is the first dissociation constant for a diprotic acid, H2A and Ka2 is the second dissociation constant for the conjugate of the diprotic acid, HA". For example, the ion HC2O4 is derived from the diprotic acid H2C2O4. H2C2O4 has first and second dissociation constants of Kal = 5.6x10-² and Ka2 = 5.1x10-5. pKal = 1.25 and pKa2 = 4.29. So to find the pH of a salt solution containing this ion, use the above equation. 1.25+ 4.29 pH = = 2.77 Certain metal ions can also affect the pH of a solution. They do this by first forming a hydrated complex ion. If the metal ion is sufficiently small in size and/or highly positively charged, then a hydrogen ion from one of the water molecules can detach resulting in an acidic solution. For example, Zn2+ forms the complex Zn(H2O)6²+ in aqueous solution. It can then react as follows. Zn(H2O)62+ + H2O S Zn(H2O)5(OH)* + H3O* Ka = 2.5x10-10 The hydronium ion concentration can then be determined using a simple ICE calculation and from there the pH determined. If neither ion in a salt affects the pH, then the solvent water is the only substance that affects the pH and will give a pH = 7. In rare cases, both ions may affect the pH if the cation is the conjugate acid of a weak base AND the anion is the conjugate base of a weak acid. In this case, a general determination of acidic, 18
Expert Solution
Step 1

Potassium carbonate is a basic salt that is formed weak acid and strong base. That is it formed from reaction between KOH and H2CO3. Therefore, the salt is alkaline in nature.

Carbonic acid is a diprotic acid. Therefore, it will undergo two dissociations and release a proton and a conjugate base during each dissociation. Similarly, the conjugate base carbonate ion CO32- will undergo two base dissociations.      

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