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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- 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)?
- 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 remainingplease explain then give answerANSWER 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…
- Calculate 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:With steps pleaseWhich 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" 00
- NoneA weak acid indicator HIn is blue while its conjugate base In is green. Kaln for the indicator is 5.1 x 10-5 Over what pH range does the indicator change color? lower pH upper pH What is the [H*]in a solution with pH =13.0? |(M) [H*]A buffer is made up of equal volumes (513.8 mL of each) of 0.846 M A H and 0.845 M A minus. 15.54 mL of 0.404 M N a O H is added to the buffer. How many moles of A H are present after the addition of N a O H? Please use correct significant figures. Answer: 0.428 M