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10.(5 points) You create a solution by placing 15.00 mL of 0.0242 M HNO, in a...
Calculate the concentration of a solution prepared by adding 15.00 mL of 1.98 × 10 −...
Calculate
the concentration of a solution prepared by adding 15.00 mL of 1.98
× 10 − 3 M K M n O 4 from a buret into a 50.00 mL volumetric flask,
which is then filled to the 50.00 mL graduation mark with distilled
water
1. Calculate the concentration of a solution prepared by adding 15.00 mL of 1.98 x 10-3M KMnO, from a buret into a 50.00 mL volumetric flask, which is then filled to the 50.00 mL graduation...
A buffer solution is prepared by placing a 25.00 mL aliquot of 0.165 M NH3 and...
A buffer solution is prepared by placing a 25.00 mL aliquot of 0.165 M NH3 and a 25.00 mL aliquot of 0.150 M NH4Cl into a 100.00 mL volumetric flask and diluting to the mark. Using activities, calculate the pH of the buffer solution. Use the Davies equation to determine activity coefficients. (pKa of NH4+ = 9.245)
Please answer within 40 minutes for when the question is due, thank you! |-/0.5 points GVSUCHEM116V2...
Please answer within 40 minutes for when the question
is due, thank you!
|-/0.5 points GVSUCHEM116V2 14.6.3.P004. My Notes Calculating the pH of a Buffer Solution To prepare a buffer you weigh out 9.00 grams of KNO2 and place it into a 500.00 mL volumetric flask. To this flask you add 18.0 mL of 3.80 M HNO, and then fill it about halfway with distilled water, swirling to dissolve the contents. Finally, the flask is filled the rest of the...
A stock solution of Cu2+(aq) was prepared by placing 0.9157 g of solid Cu(NO3)2∙2.5 H2O in...
A stock solution of Cu2+(aq) was prepared by placing 0.9157 g of solid Cu(NO3)2∙2.5 H2O in a 100.0-mL volumetric flask and diluting to the mark with water. A standard solution was then prepared by transferring 2.00 mL of the stock solution to a second 25.00-mL volumetric flask and diluting to the mark. What is the concentration (in M) of Cu2+(aq)in the stock solution? What is the concentration (in M) of Cu2+(aq)in the standard solution?
Pour 2.5 mL of the 1M glucose (C6H12O6) solution from the flask into the 100 mL...
Pour 2.5 mL of the 1M glucose (C6H12O6) solution from the flask into the 100 mL volumetric flask. Use the “dilution equation” to determine the volume in mL for the required 0.025M solution, given that the original solution is 1M and you used 2.5 mL Fill the volumetric flask to the 100 mL mark with distilled water. Note: The flask already contains a volume of 2.5 mL. 1. Compute the volume of the diluted 0.025 M solution. 2. What volume...
Determine the pH of a solution when 24.1 mL of 0.029 M HNO, is mixed with...
Determine the pH of a solution when 24.1 mL of 0.029 M HNO, is mixed with 18.6 mL of A. 0.0060 M NaOH. pH = B. distilled water. pH = C. 0.0100 M HCl. pH = D. 0.072 M KOH. pH =
A chemist must prepare 250.0 ml of hydrochloric acid solution with a pH of 1.80 at...
A chemist must prepare 250.0 ml of hydrochloric acid solution with a pH of 1.80 at 25°C. He will do this in three steps: Fila 250.0 ml. volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (6.0 M) stock hydrochloric acid solution and add it to the flask. . Fill the flask to the mark with distilled water, Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second...
in the preparation of the standard Beer's law curve, 5.00 mL, 10.00 mL, 15.00 mL and...
in the preparation of the standard Beer's law curve, 5.00 mL, 10.00 mL, 15.00 mL and 20.00 mL of a 0.108 M stock solution of glucose were added to separate 50 mL volumetric flasks. Afterwards, each of the flasks was filled to the mark with distilled water and labelled A, B, C and D accordingly. What is the concentration of glucose in the flask C? Report your answer to 3 decimal places.
A student pipets 5.00 mL of a 5.103 M aqueous NaOH solution into a 250.00 mL...
A student pipets 5.00 mL of a 5.103 M aqueous NaOH solution into a 250.00 mL volumetric flask and dilutes up to the mark with distilled water. What is the final molarity of the dilute solution? Select one: A. 0.1 MX B. 0.10206 M C. 0.102 M D. 0.1021 M Your answer is incorrect. 86.14 mL of an acid solution was needed to neutralize 30.24 mL of a base solution of unknown concentrations. A second trial is run but this...
A buffer is prepared by mixing 200.0 mL of 0.1500 M NaOH with 200.0 mL of...
A buffer is prepared by mixing 200.0 mL of 0.1500 M NaOH with 200.0 mL of 0.200 M CH3CO2H in a 1-L volumetric flask and then diluted to volume with distilled deionized water. Calculate the pH of the buffer. Ka = 1.75 x 10-5
Calculate
the concentration of a solution prepared by adding 15.00 mL of 1.98
× 10 − 3 M K M n O 4 from a buret into a 50.00 mL volumetric flask,
which is then filled to the 50.00 mL graduation mark with distilled
water
1. Calculate the concentration of a solution prepared by adding 15.00 mL of 1.98 x 10-3M KMnO, from a buret into a 50.00 mL volumetric flask, which is then filled to the 50.00 mL graduation...
Please answer within 40 minutes for when the question
is due, thank you!
|-/0.5 points GVSUCHEM116V2 14.6.3.P004. My Notes Calculating the pH of a Buffer Solution To prepare a buffer you weigh out 9.00 grams of KNO2 and place it into a 500.00 mL volumetric flask. To this flask you add 18.0 mL of 3.80 M HNO, and then fill it about halfway with distilled water, swirling to dissolve the contents. Finally, the flask is filled the rest of the...
Determine the pH of a solution when 24.1 mL of 0.029 M HNO, is mixed with 18.6 mL of A. 0.0060 M NaOH. pH = B. distilled water. pH = C. 0.0100 M HCl. pH = D. 0.072 M KOH. pH =
A chemist must prepare 250.0 ml of hydrochloric acid solution with a pH of 1.80 at 25°C. He will do this in three steps: Fila 250.0 ml. volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (6.0 M) stock hydrochloric acid solution and add it to the flask. . Fill the flask to the mark with distilled water, Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second...
A student pipets 5.00 mL of a 5.103 M aqueous NaOH solution into a 250.00 mL volumetric flask and dilutes up to the mark with distilled water. What is the final molarity of the dilute solution? Select one: A. 0.1 MX B. 0.10206 M C. 0.102 M D. 0.1021 M Your answer is incorrect. 86.14 mL of an acid solution was needed to neutralize 30.24 mL of a base solution of unknown concentrations. A second trial is run but this...
A buffer is prepared by mixing 200.0 mL of 0.1500 M NaOH with 200.0 mL of 0.200 M CH3CO2H in a 1-L volumetric flask and then diluted to volume with distilled deionized water. Calculate the pH of the buffer. Ka = 1.75 x 10-5
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