A 10.00 ml. sample of Y(OH)2 was titrated to the stoichiometric point with 14.50 ml of 0.2345 M H2X. The total number of moles of Y(OH)2 is O a. 0.00469 O b. 0.0068 Oc. 0.00034 O d. 0.0034
Q: Concentration of DDT (molar mass= 354.49 g/mol) in groundwater sample is found to be 0.030 mg/250.0…
A: We have to predict the concentration in mmol/L.
Q: To lower the concentration of a solution, we use the process of dilution, or adding more solvent to…
A: 1.MinitialVinitial = MfinalVfinal
Q: How many moles of Ca(OH) 2 are required to completely react with 300.0 L HCl solution? (HCl content…
A: Given that: Volume of HCl solution = 300 L = 300000 ml and density = 1.2 g/ml So mass of solution =…
Q: A 0.137 g sample of KaCr2O, is added to 135 mL of water. What is the concentration of the solution?…
A:
Q: Calculate the volume in (mL) required to prepare 50.0 ml that are 0.0535 M in NO, Trom a 7.88%(w/w)…
A: The question is based on the concept of molarity. it is defined as number of moles of solute…
Q: 16.792 g of Ba(OH)2 (171.342 g.mol-1) is weighed out and carefully dissolved to make a 500.00cm3…
A:
Q: 3.00- g sample of an alloy of Pb Lead was dissolved in nitric acid (HNO3). Sulfuric acid was added…
A: First Calculate mole by dividing Molar mass to the mass Then use mole -mole relationship to get…
Q: How many grams of PbBr2 will precipitate when excess NaBr solution is added to 66.0 mL of 0.609 M…
A: Hello. Since the question contains multiple parts, the first part is solved. In case the solution…
Q: The concentration of urea in a solution prepared by dissolving 16 g of urea in 36 g of H2OH2O is…
A: In order to calculate the mass % of urea we have to first write down the given data: Mass of…
Q: A KO B. CH. C co, D. P,O, 02 How many grams of Ca(OH), are required to neutralize 1000 L of 0…
A: Oxidation can be defined as the process of loss of electrons and reduction is a process of gain of…
Q: How many grams of PbBr2 will precipitate when excess NiBr2 solution is added to 57.0 mL of 0.520M…
A: Given Chemical equation :: Pb(NO3)2(aq) + NiBr2(aq) --> PbBr2(s) + Ni(NO3)2(aq)
Q: 10. A 0.514 gram sample of NażCO, (106.0 g/mol) was dissolved in distilled water in a 100.0 mi.…
A:
Q: Write the balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous NaI. Include phases.…
A: A chemical reaction in which the elements present on the reactant side and product side are equal is…
Q: A mixture is prepared by adding 25.5 mL of 0.200 M Na3PO4 to 37.7 mL of 0.126 M Ca(NO3)2. (a) What…
A: Given: The volume of Na3PO4 (V1)= 25..5 mL = 0.0255 L The volume of Ca(NO3)2 (V2)= 37.7 mL = 0.0377…
Q: How many grams of Ag,CO3 will precipitate when excess (NH4)½CO3 solution is added to 57.0 mL of…
A: Given Molarity of AgNO3 = 0.561 M = 0.561 mol/L Volume = 57 mL…
Q: How many grams of Ag2CO3 will precipitate when excess Na2CO3 solution is added to 45.0 mL of 0.538M…
A:
Q: Ammonia (NH3, MM 17.031 g/mol) and hypobromite (OBr−) react according to the following chemical…
A: Mass of ammonia = 0.423 g. Molar mass of ammonia = 17.031 g/mol. Volume of solution = 27.3 ml ....Or…
Q: A 0.750 g sample of finely ground limestone was placed in an Erlenmeyer flask, and 25.00 mL of 1.00…
A: Mass of sample = 0.750 grams Volume of HCl added = 25.0 mL Concentration of HCl added = 1M Volume of…
Q: 47.8 mg of silver nitrate (AGNO3, 169.9 g/mol) was dissolved in water to make 10.00 mL of solution.…
A: Given information is as follows: The mass of silver nitrate = 47.8 mg = 47.8×10-3 g The volume of…
Q: The mass percentage of chloride ion in a 25.00-ml sample of seawater was determined by titrating the…
A: The balanced reaction for the formation of silver chloride precipitate from silver nitrate can be…
Q: How many grams of Ag2CO3 will precipitate when excess (NH4)2CO3 solution is added to 45.0 mL of…
A:
Q: A 249.3-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first…
A: Given the mass of groundwater sample taken for analysis = 249.3 g mass of Ca2P2O7 precipitate…
Q: 73. The hardness of water (hardness count) is usually expressed in parts per million (by mass) of…
A: 1 mol CaCO3 gives 1 mol of Ca2+.
Q: If 150.0 mL of 2.5 mol/L Na2SO4 is mixed with 125 mL of 0.26 mol/L AgNO3, determine the…
A: A question based on mole concept that is to be accomplished.
Q: 5 ml of substance (A) is titrated with 38 ml of 0.1 M of substance (B). if the legal minimum percent…
A: Volume of A = 5 mlVolume of B = 35 mlMolarity of B = 0.1 Mdensity of A = 19/mlMo.wt of A = 61…
Q: A 10.00 mL of vinegar solution is titrated with 39.0 mL of 0.20 M NaOH.The calculated mass percent…
A: The question is based on the concept of quantitative analysis. we have to calculate density of the…
Q: How many grams of PbBr2 will precipitate when excess NaBr solution is added to 59.0 mL of 0.751 M…
A: As the NaBr is present in excess amount the yield of reaction is depend upon the moles of Pb(NO3)2 .…
Q: What mass of Na2SO4 (in grams) will be formed by the addition of 14.4g of NaHCO3 in aqueous solution…
A:
Q: How many grams of Ag2CO3 will precipitate when excess (NH4)2CO3 solution is added to 74.0 mL of…
A: The reactant molecule that has less number of moles than the other reactant molecules and which…
Q: If 44.97 mL HCl = 43.76 mL NaOH, and if 49.14 mL NaOH neutralizes 0.2162 g of KHC2O4.H2C2O4.2H2O,…
A: Acid and base react with each other forming salt and water. This reaction is termed as…
Q: How many grams of Ag2CO3 will precipitate when excess (NH4)2CO3 solution is added to 62.0 mL of…
A: 1- First we will determine the moles of AgNO3 : moles of AgNO3 = [ Molarity × Volume ] moles of…
Q: Phosphate in wastewater samples can be precipitated out as Ca10(PO4)6(OH)2 (1,004.6 g/mol).…
A: Given that phosphate in wastewater samples can be precipitated out as Ca10PO46OH2.And municipal…
Q: The aluminum (AW=26.98 g/mol) in a 1.000-g sample of impure ammonium aluminum sulfate was…
A:
Q: Ammonia (NH,, MM 17.031 g/mol) and hypobromite (OBr") react according to the following chemical…
A:
Q: How many grams of Ag2CO3 will precipitate when excess Na2CO3 solution is added to 41.0 mL of 0.744 M…
A:
Q: How many grams of PbBr2 will precipitate when excess NaBr solution is added to 72.0 ml of 0.791 M…
A:
Q: ) A 1.20 gram sample of ammonium phosphate is dissolved in 100. mL of water. The solution is poured…
A: The balanced equation is 2(NH4)3PO4 (aq) + 3 Mg(NO3)₂(aq) --> Mg3(PO4)₂ (s) + 6NH4NO3(aq) Net…
Q: excess silver nitrate is added to 100.0 mL of a solution containing barium ions to produce 1.84 g of…
A: C. 1.28 x 10 -1 M
Q: Part A A sample of 7.92 g of Mg(OH)2 is added to 24.2 mL of 0.225 MΗΝΟ, Part B Part C • Part D •…
A:
Q: A sample of ore containing manganese weighed 1.2354 grams. This sample was heated in a solution of…
A: Initially we are calculating number of Mn2S3 and from that number of moles of Mn(NO3)3 is calculated…
Q: 16.792 g of Ba(OH)2 (171.342 g.mol-1) is weighed out and carefully dissolved to make a 500.00cm3…
A:
Q: 5 ml of substance (A) is titrated with 38 ml of 0.1 M of substance (B). if the legal minimum percent…
A: Molarity of substance A can be calculated using the relation: M1V1=M2V2 from molarity, moles of A…
Q: Write the balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous NaI. Include phases.…
A: According to the solubility rule, PbI2 is an insoluble compound. Hence, the reaction between aqueous…
Q: mol M = L %3D A solution is made from 0.315 mol of Na Cr207. If the volume of the solution is 25mL,…
A: In this question, we want to determine the Molarity of the Na2Cr2O7 Solution. How we can determine…
Q: A (aq) + ....B(aq) Č(s)+ D (aq) Experimental Volume of B/ mL Mass of Run precipitate/g 1 1.2 5.40 2…
A:
Q: 16.792 g of Ba(OH)2 (171.342 g.mol-1) is weighed out and carefully dissolved to make a 500.00cm3…
A:
Q: How many grams of Al are needed to produce 0.450 L of 1.6 M solution of AICI3? 2AI + 6HCI → 2AICI3 +…
A: Given-> Volume of AlCl3 = 0.450 L Molarity = 1.6 M
Q: what mass of ammonium sulfate could you produce?
A: Molarity = number of moles/volume of solution (in L) Number of moles = molarity × volume(in L)…
Q: What volume of 0.032 M AgNO3 can be made from 3.8 g AgNO3?
A:
Hi! Please answer B and C.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
- A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3 . Express the results of this analysis in terms of the percentage of BaCl2 * H2O. (Use a MW value in 4 decimal places)(a) For the precipitation reaction: A+ + B– AB(s)Calculate the value of the equilibrium constant for 99.99% conversion to AB atthe equivalence point, assuming that the analyte content is 5.00 mmole and thetotal volume at the equivalence point is 100.00 mL.(b) What factors affect end-point sharpness in a precipitation titration? Explain.(c) Explain briefly why silver nitrate is an important reagent used in precipitationtitrations.(d) Mohr Method, Volhard Method and Fajans Method are commonly used for thevolumetric analysis of chlorides. Distinguish the three methods in terms of thetitrants and indicators used, and how the titrations are carried out.
- A sample is analyzed for chloride by the Volhard method. From the following data, calculate the percentage of chloride present:Weight of sample = 6.0000 g dissolved and diluted to 200 mLAliquot used = 25.00 mL AgNO3 added = 40.00ml of 0.1234MKSCN for back titration = 13.20ml of 0.0930MCrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42- should be used so that Ag2CrO4(s) just starts to form at the equivalence point? If a concentration of 0.0010 M CrO42- is used instead, at what concentration of Br- will Ag2CrO(s) just start to precipitate? Do you think this is likely to introduce significant error? The Ksp for Ag2CrO4(s) is 1.2x10-12.Chemistry A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this solution is taken and titrated with 0.05 M EDTA at pH = 10 in the presence of Erio – T indicator, the consumption is found as 12 mL. A new 10 mL was taken from the same solution and (NH4)2C2O4 is added on it and then formed the precipitate is filtered. The filtered solution is titrated with the same EDTA solution and the consumption is found as 3 mL. So find the Ca2+ and Mg2+ amounts in the main sample solution in terms of mg/L.
- Which of the following statements is advantageous? A). The main differences between potentiometric and conductometric titrations are that potentiometric titrations exemplify the analyte sample-by-sample while conductometric titrations show the potential of the analyte B). A conductivity is analyl from the people of the charge. C.) Conductivity increases rapidly as close as equivalence, as a strong acid and a strong base will decrease D). The conductor remains constant according to the viscosity of the pixel, the decomposer and its size, which consists of design modelling.The % (w/w) I- (MM = 126.9) in a 0.5812-g sample was determined by Volhard titration. After adding 50.00 mL of 0.06912 M AgNO3 and allowing the precipitate to form, the remaining silver was back-titrated with 0.07012 M KSCN, requiring 36.17 mL to reach the endpoint. Report the %(w/w) I- in the sample. 35.52 % 20.08 % 17.76 % 40.16%1ml of 1mg/ml of diluted aspirin powder solution is titrated by 0.005M NaOH. Before titration, 5 ml ethanol, 14 ml CO2 free water, and 4 drops bromothymol blue indicator is added into diluted aspirin powder solution. Mass of 0.005M NaOH used is obtained by weight titration = 1.1384g . [Molar mass of aspirin =180.15]; for solution, 1g=1mL at 25 degree Celcius. Calculate the purity of the powder.
- volumetric or graduated piptte, Which one of them is commonly used for Titration and reagent and which one is more accurate, why?What volume (V) of 0.100M (moles) KMnO4 would be required to Titrate 0.23g of K2{Cu(Cu2O4)2} * H20?How would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should precipitate when 5ml of 0.0040 M AgNO3 are added to 5ml of 0.0024 M K2CrO4. You can come up with your own experimentally Ksp value. I just want to see steps in solving