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What is the physiological pH and A- /AH ratio for the following graph...
![Titration Curve of Plasma
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[NaOH] mM
Hd](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa77d439e-6e4f-4050-a6c7-d8833fccbd3e%2F3d010b36-9959-4085-b9df-8da289b1b3f8%2F75wj7u4_processed.png&w=3840&q=75)
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- help find titration concentration from given data (use sig figs please)2. Below is a titration curve generated by a similar titration to the ones simulated, Vinegar Titration Curve 14.00 13.00 12.00 11.00 10.00 9.00 8.00 * 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 Volume NaOH (mL) We can use this curve to estimate the pka of our weak acid by what is called the "half equivalence point method". The equivalence point is the middle of the steepest part of this graph. Estimate the volume of NaOH added to the titration at that point by using a rule or other straight edge to follow that point down to the x-axis. Divide that volume by 2 (half the equivalence point) and estimate the pH at that volume of NaOH using your straight edge again. pKa = pH at the half equivalence point. What do you estimate the pka to be? 3. The pka of acetic acid is 4.76. Calculate percent error between the true value and your estimated value from question 2.What volume (mL) of 0.2173M NaOH is required to titrate 50.00mL of 0.2980M HCI ?In the titration of 50.00mL of 0.2980M HCl. 71.93mL of 0.2173M NaOH was required to reach the phenolphthalien endpoint. Calculate the percent error between the predicted amount and the experimental amount. What does this tell you about the concentration of the NaOH? This is based on your answers to questions 1 and 2. Question 3 options: The concentration of the NaOH is 0.2173M. The concentration of the NaOH is stronger that 0.2173M. Nothing new The concentration of the NaOH is weaker than 0.2173M. Please answer fast i give upvote.
- Using the derived endpoints for both phosphoric acid titrations, calculate theconcentration of the phosphoric acid solution and report the mean value. Vol Mid Point 1st Derivative 3.96 0.089821268 5.91 0.229138878 7.105 0.257152358 8.345 0.562805368 9.025 1.958394009 9.175 4.406074475 9.215 10.52631579 9.27 5.043426253 9.355 4.129394633 9.415 7.738714375 9.465 2.260096883 9.505 13.04347826 9.605 1.258033788 9.8 0.85812357 10 0.845641773 10.25 0.636571666 10.65 0.415019763 11.2 0.31048471 11.95 0.277373275 12.925 0.270438943 13.875 0.273865319 14.55 0.391304348 15.025 0.421607378 15.425 0.567030224 15.7 0.934574579 15.9 0.898689411 16.05 1.831703765 16.125 4.911587269 16.175 4.137715831 16.25 3.061160807 16.325 7.932182234 16.375 6.403162055 16.45 3.070522155 16.55 1.981485334 16.675 1.751612232 16.875 0.8562513 17.075 1.352194716 17.375 0.427848277 17.85 0.434990639 18.475 0.249635948 19.275…10.0 mL of NaOH solution with unknown concentration is titrated with 0.10 M of HCl solution in the presence of phenolphthalein indicator. At the end of the titration 15.0 mL of HCl solution is used. What is the number of millimoles and concentration of NaOH solution used? A. 1.5 mmol and 0.15 M NaOH B. 1.0 mmol and 0.15 M NAOH C. 1.5 mmol and 0.1 M NaOH D. 2.0 mmol and 0.1 M NaOH E. 1.0 mmol and 0.1 M NaOH Which of the following statements is false for the reactions given below: Cr* + Sn4+ → Cr³+ + Sn²+ 2As(s) + 3C2(g) → 2ASCI3 3Hg2+ + 2Fe(s) → 3Hg2 + 2FE3+ A. Sn+4 is reduced. B. As gains electrons. C. Cr* → Cr3+ half reaction takes place in the anode. D. As(s) is oxidized. E. Hg2+ → Hg2 half reaction takes place in the cathode.Would you calculate the ionic strength of this buffer? [Na2HPO4]=.024176 [NaH2PO4]=.1
- Why is titrant added rapidly at the beginning of titration but more slowly as titration proceeds?Construct a titration curve from the data below. Determine the volume of titrant at equivalence point.The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution with 0.0700 M KOH. 1) What is the initial pH of the analyte solution? 2) What volume of KOH is required to reach the equivalence point of the titration (in mL)? 3) How many mmol of the salt are present at the equivalence point? (ANALYTICAL AMOUNT, NOT EQUILIBRIUM AMOUNT) 4) What is the volume of the solution at the equivalence point (in mL)? 5) What is the molar concentration of the salt at the equivalence point? (ANALYTICAL CONCENTRATION, NOT EQUILIBRIUM CONCENTRATION) 6) What is the pOH at the equivalence point? 7) What is the pH at the equivalence point? 8) How many mL of KOH have been added at the half-equivalence 9) What is the pH at the half-equivalence point?
- Use the volumes and pH calculated to plot a titration curve. Label the axis and identify on the graph the equivalence point and the half way equivalence point for the titration. A) 0mL pH=2.98 B) 10mL pH=4.44 C) 12.5mL pH=4.57 D) 25.0mL pH=5.04Define the end point of a titration: a) It is a synonym for equivalence point b) It is when a change that indicates equivalence is observed in the analyte solution c) It is the point at which the pH no longer changes29 In GC, the sample injected in liquid state vaporizes inside the column. * True False 30 In GC, the sample is carried through the column by inert gas. True False
