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A: Given data,Number of B atoms=3.6×1024atomsMolar mass of B=10.811g/mol
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- Potentiometric Complexometric Titration Of Ca and Ma We want Aim Theory Material chemical used Procedure of analysis Data and calculationWhich one is not the correct experimental condition for complexometric titration?a) Need strong complexing agent than indicatorb) Basic buffer solution of pH 8 is requiredc) Titration must be done at room temperatured) Small amount of Mg2+ must be added to titrante) Complexometric indicator must be used.Within what pH range is a HOCl – NaOCl buffer effective? Answer: pH 6.5 – pH 8.5 (Please explain. Thank you.)
- ANSWER BI AND ANY OTHER THREE QUESTIONS SECTION D Question B1 One way to delermine the pKa value is by use ofa pli curve. One student used thie pH curve to determine thc pka value of the weak monoprotic acid. She transferred 25.0 cm' of 0.100 M solution of the acid into a conical flask and measured the pll of the acid solution using a pH mcter accurate to one decimal place. A solution of sodium hydroxide of concentration 0.100 mol dni was added from the burette in small portions until the alkali was present in excess. The pH of the mixture was recorded after each addition of the sodium hydroxide solution. Then she plotted the pH of the solution versus volume of alkali added from the burette and used this graph to determine the acid dissociation constant. 14 12 10- 10 20 30 40 50 VNaOH (ml) a) Calculate mass of the acid required to prepare 100 cm' of 0.1 solution of this acid.(Molar mass of the acid 150 g mol) b) What is the volume of sodium hydroxide added at cquivalence point? c) What…ollowing statements is incorrect A) Standardization is required when the titrant solution molarity is approximate B) A standard solution should react completely with the analyte. C) A secondary standard should be highly pure (99.99%). D) Back-titration is required when the rate of the reaction slow. E) Titration error is the difference between equivalence point volume and end point volume.Question 7 Volhard method is supported by the following statements EXCEPT Choose the best answer. Titration can be done even at a pH lower than 6.5 The endpoint of the back titration is the formation of a colored complex ion. Involves the addition of excess AgNO3 to a halide solution, followed by back titration of the excess by KSCN The acidic pH condition prevents the appearance of the green suspension at endpoint.
- Question 24 of 27 What ratio of NaCN to HCN is needed to prepare a pH 10.00 buffer? (Ka of HCN is 4.9 x 10 10) +/- image_6487327.JPGDescribe the information necessary (and why) to choose a good indicator for a weak acid/strong base titration. Answer:Review Topics Use the References to access important values if needed for this question. The pK, value for H2S is 7.00. What mole ratio of KHS to H2S is needed to prepare a buffer with a pH of 6.80? HS [H2 S] Submit Answer Retry Entire Group 9 more group attempts remaining
- Question 5 Acetic acid is a convenient buffer system in the slightly acidic range. What mass of sodium acetate (NaCH,CO,) must be added to 0.750 L of 0.129 M solution of acetic acid to make a buffer of pH = 5.00? The K, of acetic acid is 1.8E-5. 9. The number of significant digits is set to 3; the tolerance is +/-1 in the 3rd significant digit How many moles of acid are required to change the pH of the solution in part a by 0.05 pH units? mol The number of significant digits is set to 3; the tolerance is +/-1 in the 3rd significant digit LINK TO TEXT Suppose 5.0 mL of 12.0 M HCI solution is added to the buffer solution in part a. Calculate the new pH. The number of significant digits is set to 3; the tolerance is +/-2.0%If you titrate a weak base analyte with a strong acid titrant, the pH at the equivalence point would be… (a) Very basic (b) slightly basic (c) neutral (d) slightly acidic (e) very acidic If you titrate a strong base analyte with a strong acid titrant, the pH at the equivalence point would be…(a) Very basic (b) slightly basic (c) neutral (d) slightly acidic (e) very acidic If you titrate a strong acid analyte with a strong base titrant, the pH at the equivalence point would be…(a) Very basic (b) slightly basic (c) neutral (d) slightly acidic (e) very acidic If you titrate a weak acid analyte with a strong base titrant, the pH at the equivalence point would be…(a) Very basic (b) slightly basic (c) neutral (d) slightly acidic (e) very acidic75. pK, of NH," is 9.26. Hence, effective pH range for NH,OH-NH,Cl buffer is about :- (1) 8.26 to 10.26 (2) 4.74 to 5.74 (3) 3.74 to 5.74 (4) 8.26 to 9.26