pls solve to the weight of Calcium in mg: given: Sodium-EDTA used: 4.204 g Calcium carbonate used: 0.4050 g the average Molarity of EDTA: 0.01114M the volume used to titrate is 23.55ml and 5 ml of the buffer is added.
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Q: pls solve to the weight of Calcium in mg: given: Sodium-EDTA used: 4.204 g Calcium carbonate used:…
A: Given that - Mass of sodium-EDTA used = 4.204 g Mass of Calcium carbonate used = 0.4050 g The…
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- ind the pH of the equivalence point(s) and the volume(mL) of 0.0372 M NaOH needed to reach it in titrations of(a) 42.2 mL of 0.0520 M CH₃COOH(b) 28.9 mL of 0.0850 M H₂SO₃(two equivalence points)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 acidicWhich 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.
- Need solution urgently 125mL of an alkaline water sample containing 128 ppm carbonate and 40ppm hydroxide in terms of CaCO_(3) equivalent its titrated against 0.20NHCl using methyl orange as the indicator.What will be the titre value (in ml unit)?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…Within what pH range is a HOCl – NaOCl buffer effective? Answer: pH 6.5 – pH 8.5 (Please explain. Thank you.)
- 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 remainingWhich of the following statement regarding EDTA titration is incorrect* Mark only one oval. (HOS HOSM O In normal direct titration, the color of the endpoint is from the metal-indicator complex In back titration, excess EDTA is titrated with another standard solution of a HOa second metal ion In indirect titration, the analyte can not be titrated against EDTA In masking titration, the sample or the interference can be isolated by "masking" 00Calculate the pH of a NH4*/NH3 buffer that was prepared with 100.0 mL of 0.500 M NH4CI and 50.0 mL of 0.400 M NH3 solution. (K, for NH3 is 1.76x10-5) Answer:
- Which indicator could be used to titrate aqueous NH3 with HCl solution? Acid Color- Indicator Range Change pH Color (a) pink 1.2 2.8 (b) blue 3.4 4.6 (c) yellow 6.5 - 7.8 (d) colorless 8.3-9.9 none of (e) these A D EA lactic acid/lactate ion buffer solution contains 0.11 M HC3H;O3 and 0.78 M C3H;O3-, respectively. The Ka value of lactic acid is 1.4 x 10¬4. Calculate the pH of this buffer. Express the pH numerically. • View Available Hint(s) ? pH = SubmitA buffer solution contains 0.487 M CH,NH,Cl and 0.252 M CH,NH, (methylamine). D the pH change when 0.058 mol KOH is udded to 1.00 Lof the buffer. etemine pH ater addition - pli before addition- pH change-( Submit Answer Retry Entire Group more group attempts remaining Determine the pHi change when 0.080 mol HCIO, is added to 1.00 Lof a buffer solution that is 0.340 M in CH,COOH and 0.283 M in CH,COO". pH after addition - pH before addition pl change -[ Submit Answer Retry Entire Group 9 more group attempts remaining