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- Situation: A 0.1214-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.07011 M AgNO3, the sample was back titrated with 0.06021 M KSCN, requiring 27.15 mL to reach the end point. What is the net ionic equations involved of the above titration process?A student weighs 0.3745 g of unknown and dissolves it in 45 mL of water. A 0.1125 M solution of HCl is used as a titrant. When the halfway point (phenolphthaleincolor change) of the titration is reached, the volume of HCl used is 17.21 mL. What is the estimated % Na2C03in the student's unknown?Determine the molar solubility ( ? ) of Ag2CO3 in a buffered solution with a pH of 5.835 using the systematic treatment of equilibrium. ?sp(Ag2CO3)=8.46×10−12 ; ?a1(H2CO3)=4.45×10−7 ; ?a2(H2CO3)=4.69×10−11 .
- What species are present in a solution giving off a pure blue endpoint in a hard water sample containing an EBT indicator (In) with an EDTA titrant? a. HIn²⁻, CaY²⁻, MgY²⁻ b. HIn²⁻, MgIn⁻, CaY²⁻, MgY²⁻, CaIn⁻ c. HIn²⁻, MgIn⁻ d. HIn²⁻, MgIn⁻, CaY²⁻An unknown sample weighing 0.2583g is titration to the end point with 47.28mL of a 0.10M AgNO3 solution. What is the weight percent of Cl- in the sample?2. Calculate tirimetric conversion factor of titrant – sodium tiosulphate (M=158,11 g/mol)corresponding to iodine (М=253,809 g/mol), if molar concentration of the salt is 0,1045 mol/l. Express numerical result with an accuracy of: Х,ХХХХХ
- A. Why is the titration of the oxalate in the green salt with KMnO4 performed prior to carrying out the redox titration for iron content? (Why can’t you do them the other way – iron first then oxalate?) B. In a titration using 0.02000 M KMnO4 solution, the following data were obtained: Buret readings: FINAL = 15.31 mL INITIAL = 5.02 mL How many moles of KMnO4 were used?Situation: A 0.1214-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.07011 M AgNO3, the sample was back titrated with 0.06021 M KSCN, requiring 27.15 mL to reach the end point. Questions: ONLY answer NUMBERS 3 and 4 Write the net ionic equations involved of the above titration process. Calculate the purity of the Na2CO3 sample based on the given above. The Ksp of AgCl is 1.82 x10-10 and the Ksp of AgSCN is 1.1 x10-12. Calculate the molar solubility of each express as mol Ag+/ L. What precipitate is more soluble? Is there a problem with this with reference to the titration above? And if there is, how will you remedy this?A sample consisting of Na2CO3, NaOH and inert matter weighs 1.179g. It is titrated with 0.2239M HCl with phenolphthalein as the indicator. The solution became colorless after the addition of 45.62 mL. Methyl orange is then added and 12.85 mL more of the acid are needed for the color change. what is the percent Na2CO3 in the sample?
- The solubility of Ag2CrO4 is 0.024 g/L. Determine Ksp for silver chromateCalculate [Cr3 + ] in equilibrium with Cr(OH)4-(aq) when0.010 mol of Cr(NO3)3 is dissolved in 1 L of solution bufferedat pH 10.0.A 25.00 mL solution of 0.08960 M NaI is titrated with 0.05040 M AgNO3. Calculate pAg+ following the addition of the given volumes of AgNO3. The ?sp of AgI is 8.3×10−17 .35.20 mLpAg+= ?epAg+= 46.40 mLpAg+=