Standard CaCO, is used to standardize the EDTA solution prior to titration. Suppose 0.385 g of CaCO, was dissolved and diluted to 250.0 mL. A 25.0 mL aliquot of this standard CaCO3 solution was then titrated to endpoint using 29.50 ml. of the EDTA solution. Afterwards, the standardized EDTA solution was used to analyze the hardness of a 1000-ml water sample buffered at pH 10. The sample required 44.35 ml. of the EDTA solution to reach the endpoint. Determine the hardness of the sample in ppm CaCO3.
Q: Write the complete electron configuration for the common monatomic ion formed by the element…
A: Given that - Monoatomic atom = Bromine , Br It is the third element of halogen group. It has…
Q: The following stands for the frequency factor in the Arrhenius equation. Ea R A k
A:
Q: What is the solubility (in mol/L) of PbCl₂ given that the Ksp is 5.13-10-8 Question Help: Message…
A:
Q: What is the pH of the solution when Julianna has added 15.00 mL of the 0.50 M HCl to the 40.00 mL of…
A:
Q: In the proposed two-step mechanism of decomposition of ozone the oxygen is: step 1: O3=>O2 + O…
A: In the given the reaction mechanism of a question is given and the role of oxygen in this reaction…
Q: predict the reaction type (single or double displacement) -- predict the names and states of the…
A: Given that, Copper metal + aqueous silver nitrate
Q: please do this typewritten, so everything is visible. thank you I will upvote only if typewritten.
A: c) part answer
Q: Calculate the molarity of a solution prepared by dissolving 22.46 grams of LiF (OR Li F) to total…
A:
Q: What is the pH of the original 0.400 M propionic acid solution? KaHA = 1.34 x 10-5 pH of 0.40 M HA =…
A:
Q: 5.81 x 10-2 b) Write the number in scientific notation: 863,000 = Use standard format to enter…
A: Ans. (a) The number is : 5.81×10-2 decimal form = 0.00581 (b) The number is: 863,000 scientific…
Q: You need to control the pH of a solution at 4.5 You have solid citric acid (pKa1= 3.13, pKa2=4.76,…
A:
Q: Consider the following hypothetical equation. A2B3 + 3 C2D --> A2D3 + 3 C2B OR A2 B3 + 3 C2 D…
A:
Q: A solution NaOH(aq) contains 6.6 g NaOH(s) per 100.0 mL of solution. Calculate the pH and…
A: The mass of solute, NaOH is = 6.6 g The volume of the solution is = 100.0 mL The molar mass of NaOH…
Q: If the ?a of a monoprotic weak acid is 2.9×10−6, what is the pH of a 0.29 M solution of this…
A:
Q: Arrange the following atoms in the order of increasing ionization energy: From lowest to highest…
A: For the ionization energy of elements, there is a trend which is a general prediction of ionization…
Q: Maria titrated 40.00 mL of 0.50 M lactic acid with 0.25 M NaOH. What is the pH of the initial acid…
A: we have to calculate the initial pH of solution
Q: What is the pH of the solution when Oscar has added 25.0 mL of 1.0 M HI to the 100.0 mL of 0.50 M…
A:
Q: If 50 ml of 1.00 M of H₂SQ and 50 ml of 2.0 M KOH are mixed what is the concentration of the…
A:
Q: NH3(aq) + H₂O(1) = NH(aq) + OH- (aq) The equilibrium hydroxide concentration in a 0.0220 M NH3…
A: Concept based on the pH calculation of the the given concentrated solution.
Q: Aqueous barium chloride + aqueous sodium sulfate Reaction Type: Balanced Equation: Product Names &…
A:
Q: Write the balanced ?a and ?b reactions for HSO−3 in water. Include physical states for each…
A: Given question is : Write the balanced ka and kb reactions for HSO3- in water. Include physical…
Q: pt of The following thermochemical equation is for the reaction of hydrogen sulfide (g) with…
A:
Q: 1. Ag₂0, NaOH 2. H₂O H
A:
Q: What is the name of the alkali metal that is in period 4? Potassium What is the name of the halogen…
A: Periodic table is arrangement of elements in horizontal rows and vertical groups.
Q: Provide the correct common name for the compound shown here. ZI
A:
Q: What is the pH of the solution when Caitlin has added 30.00 mL of the 0.25 M LIOH to the 25.00 mL of…
A: Here we are required to find the pH of the solution.
Q: What is the pH of 0.180M NH4Cl. Ka NH4+: 5.80x10^-10
A:
Q: Draw the least stable resonance form for the intermediate in the following electrophilic…
A:
Q: We can draw three inequivalent Lewis structures for the bromate ion, BrO3 structure that is the best…
A: we have to calculate the formal charge and determine the best Lewis structure
Q: 1. How many unpaired electrons are in the nitrogen atom? This atom is A. Paramagnetic B. Diamagnetic…
A: Paramagnetic substances are those which have unpaired electrons and diamagnetic substances are those…
Q: Provide IUPAC names for the given structures or structures for the given names. HN-CH₂ CI god you
A: The answer to the following question is-
Q: What is the pH of the solution when Yolanda has added 60.0 mL of 0.10 M LIOH to the 40.0 mL of 0.40…
A: we have to calculate pH of solution after addition of 60 mL base
Q: 48. For the reaction shown, find the limiting reactant for each of the initial quantities of…
A:
Q: Linda titrates 60.00 mL of 0.20 M dimethylamine, (CH3)2NH2, with 0.40 M HBr. (CH3)2NH₂ Kb = 5.4 x…
A:
Q: For each of the species below, identify any cyclic conjugated system, then: A. Determine the number…
A:
Q: 1. Consider the reaction sequence given below: Compound C 1. LDA, THF, -78°C 2. Br NaOEt Br Compound…
A:
Q: You need to make an aqueous solution of 0.140 M manganese(II) sulfate for an experiment in lab,…
A: we have to calculate mass of manganese(II) sulfate needed to prepare the solution
Q: Provide the correct systematic name for the compound shown here. CH₂CH3 CH₂CH3
A: Write the systematic name --
Q: Give the symbol of the atom with the following orbital diagram: NN 1s 2s a. b. C. 1s 2s NN 2p M 2p…
A: In the orbital diagram of an atom, we fill all the electrons present in a neutral atom. The total…
Q: HO ∞ H Br KMnO4 NaOH 0 °C 1. KMnO4, NaOH, A 2. dil. H₂SO4, H₂O 1. KMnO4, NaOH, A 2. dil. H₂SO4, H₂O…
A: Here we have to predict the major products formed in the following given reactions.
Q: What is the pH of the solution when Julianna has added 10.00 mL of the 0.50 M HCl to the 40.00 mL of…
A:
Q: 1 NaOH Halobenzenes that do not have electron-withdrawing groups can still undergo substitution…
A: Aromatic nucleophilic substitution reactions proceeds through Benzene mechanism require strong base…
Q: Jose titrated 40.00 mL of 0.25 M methylamine, CH3NH2, with 0.40 M HCI. CH3NH₂ Kb = 4.4 x 10-4 What…
A: Given data : Concentration of methylamine = 0.25 M Volume of methylamine = 40.00 mL Concentration of…
Q: 2) Draw the product of the following pericyclic reaction. light Show how you formed the product by…
A:
Q: BI2. H2O NOH HO ил
A: Since you have posted multiple questions we are answering first question for remaining question to…
Q: How can slaked lime be mixed with a percentage of the water produced to form potassium hydroxide
A: Given that - Reactant = slaked lime , Ca(OH)2 Product = potassium hydroxide , KOH If water…
Q: The percent mass of aluminum in Al(CH3COO)3 is.... %? solve.
A: I have given the answer in the explanation section. Hope you will understand that.
Q: 4. Complete the table below and answer the questions. For the Column 4, multiply [H+] and [OH-]…
A: pH is equal to the negative log of the hydronium ion concentration. pOH is equal to the negative log…
Q: 1A H 2A Li Be Na Mg 3B 4B 5B 68 7888 3A 4A 5A 6A 7A He BCN OF Ne S Cl Ar 1B 2B Al K Ca Sc Ti V Cr Mn…
A: In chemistry electronic configuration is distribution of electrons of an atom or molecule in atomic…
Q: What is the molar solubility (in mol/L) of Pb(OH)₂ (Ksp = 8.60 · 10-13) in a solution buffered at…
A: PbOH2 solution is buffered at 11.15 and the Ksp of PbOH2 is 8.60 × 10-13 .We have to calculate the…
Step by step
Solved in 3 steps with 3 images
- The concentration of a solution of EDTA was determined by standardizing against a solution of Ca2+ prepared from the primary standard CaCO3. A 0.4302g sample of CaCO3 was transferred to a 60mL volumetric flask, dissolved using a minimum of 6 M HCl solution, and diluted to volume. A 44mL portion of this solution was transferred into a 250-mL Erlenmeyer flask and the pH adjusted by adding 5 mL of a pH 10 NH3-NH4 L buffer containing a small amount of Mg2+ EDTA. After adding calmagite as a visual indicator, the solution was titrated with the EDTA, requiring 632mL to reach the end point. Calculate the molar concentration of the titrantA 0.7352g sample of ore containing Fe3+, Al3+ and Sr2+ was dissolved and made up to 500.00 mL. The analysis of metals was performed by a chemistry using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard solution of EDTA 0.02145 mol/L, requiring 6.95 mL to reach the end point. Subsequently, another 25.00 mL aliquot was buffered at pH=5 and titrated with the same EDTA solution, requiring 6.24 mL to reach the end point. Finally, a third aliquot of 25.00 mL was titrated at pH=11, requiring 11.10 mL of the same EDTA solution to complete the titration. Determine the percentage of each of the metals in the sample Given the molar masses: Fe=55.845 g/mol; Al=26.982 g/mol and Sr=87.620 g/mol.The concentration of a solution of EDTA was determined by standardizing against a solution of Ca2+ prepared from the primary standard CaCO3. A 0.4025 g sample of CaCO3 was transferred into a 250 mL Erlenmeyer flask and the pH adjusted by adding 5 mL of a pH 10 NH3-NH4Cl buffer containing a small amount of Mg2+EDTA. After adding calmagite as a visual indicator, the solution was titrated with the EDTA requiring 42.36 mL to reach the end point. Report the molar concentration of the titrant.
- A 1.509-g samle of a Pb/Cd alloy was dissolved in acid and diluted to exactly 250.0 mL in a volumetric flask. A 50.00-mL aliquot of the diluted solution was brought to a pH of 10.0 with an HCN/NaCN buffer, which also served to mask the Cd2+; 11.56mL of the EDTA solution were needed to titrate the Pb2+. Calculate the percentage of Pb and Cd in the sample.Chromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.A 0.9352g sample of ore containing Fe³+, Al³+ and Sr²+ was dissolved and made up to 500.00 mL. The analysis of metals was performed using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard 0.03145 mol/L EDTA solution, requiring 6.95 mL to reach the end point. Subsequently, another 25.00 mL aliquot was buffered at pH=5 and titrated with the same EDTA solution, requiring 6.24 mL to reach the end point. Finally, a third aliquot of 25.00 mL was titrated at pH=11, requiring 11.10 mL of the same EDTA solution to complete the titration. Given the molar masses: Fe=55.845 g/mol; Al-26.982 g/mol and Sr-87.620 g/mol. a) Determine the percentage of each of the metals in the sample. b) Explain why the change in pH allows the determination of the three ions in this sample.
- A 5.323 g of dried eggshell is transferred to a 250-mL beaker and dissolved in 25 mL of 6 M HCl. The mixture was filtered and transferred into a 250 mL volumetric flask and diluted to the mark. A 20.00-mL aliquot is placed in a 125-mL Erlenmeyer flask and buffered to a pH of 10. The mixture was titrated with 0.04992 M EDTA and 43.25 mL was consumed to reach the end point. Determine the amount of calcium in the eggshell as %w/w calcium carbonate.A salt sample was analyzed for its purity. A 0.5000g sample was dissolved in water and diluted to 250.0mL. From this solution, 25.00mL was taken for analysis. To this aliquot, 20.00mL of a 0.08735M AgNOg solution was added to precipitate the chloride. The excess AgNO, required 12.45mL of a 0.09473M KSCN solution for back-titration. Calculate the purity of the salt sample as percent by mass of KCI (74.55 g/mol). (Answer: 84.63% KCI)The amount of iron in a meteorite was determined by a redox titration using KMnO4 as the titrant. A 0.4185 -g sample was dissolved in acid and the liberated Fe3+ quantitatively reduced to Fe2+, using a reductor column. Titrating with 0.0051 M KMnO4 requires 23.44 mL to reach the end point. Determine the %w/w Fe2O3 in the sample of meteorite. (Fe = 55.845 amu, Fe2O3 = 159.69 g/mol
- An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask. and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, (a) Outline the two steps involved, representing the related reactions. (b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution. (c) Calculate the masses of CaCO3 and MgCO3 present in the pellet. (d) Calculate the…. An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, a) Outline the two steps involved, representing the related reactions./5 b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution./6 c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6 d) Calculate…c. An EDTA solution is standardized against high-purity CaCO3 by dissolving 0.3982 g CaCO3 in hydrochloric acid, adjusting the pH to 10 with ammoniacal buffer, and titrating. If 38.26 mL was required for the titration, calculate the molarity of the EDTA. (Molecular weight EDTA = 292.24 g mol-1)