.. We want to determine the purity of alum sample bought in a local pharmacy in Miagao. A Chem 28 student determined the purity gravimetrically of a sample of alum, K2SO4·Al2(SO4)3•24H20. A 1.5879-g sample was dissolved and the aluminum precipitated as Al(OH)3. The precipitate was collected by filtration, washed, and ignited to give a product Al2O3 weighing 0.1572 g. Show your calculation to determine the purity of the alum sample.
Q: One of relatively few reactions that takes place directly between two solids at room temperature is…
A: Balanced chemical equation is one in which the number of atoms of each kind is equal on both sides…
Q: The fertilizer ammonium sulfate, (NH4)2SO4, is prepared by the rxn of ammonia with sulfuric acid.…
A:
Q: Brass is an alloy consisting mainly of copper and zinc. To determine the percentage of copper in a…
A: A numerical problem based on extraction of metal from alloy, which is to be accomplished.
Q: Marble, a material used in buildings and statues, has the chemical composition CaCO₃. CaCO₃ reacts…
A: Balanced chemical reaction for the dissolution of marble is as follows: In order to calculate the…
Q: The hardness of water (hardness count) is usually expressed in parts per million (by mass) of…
A:
Q: Hydrogen peroxide solutions can easily be decomposed by dust, trace amounts of metals or light. It…
A: The balanced reaction taking place is given as, Given: Concentration of KMnO4 = 0.372 M And volume…
Q: A 1956 dime is made of a silver-copper alloy and has a mass of 2.490 g. The dime was dissolved in…
A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
Q: An environmental chemist analyzed the effluent (the released waste material) from an industrial…
A: Given : Volume of sample = 3.52 ml Volume of NaOH solution = 10.59 ml Concentration of NaOH…
Q: weighed 3.893 g of Nickel(II) Chloride Hexahydrate, dissolved it in water and reacted it with an…
A:
Q: Based on the field of civil engineering, choose particular equipment or device used, and enumerate…
A: Chromium is a metal frequently used to help alloys resist corrosion. ... Nickel is a metal often…
Q: 13.) Calculate the mass of solid MgSO̟•7H¸O that must be added to precipitate out all of the PO,3-…
A: The balanced equation for the dissociation of MgSO4.7H2O is: MgSO4.7H2O(s) → Mg2+(aq) + SO42-(aq)…
Q: In the laboratory you are given the task of separating Ca2+ and Ag* ions in aqueous solution. For…
A: The compound formed by every metal ion with another anion possesses a different solubility depending…
Q: 5. A 0.8102-g sample of impure Al2(CO3)3 decomposed with HCl; the liberated CO2 was collected on…
A: In the Question- 5 we want to determine the percentage of Al in the sample. You can see details…
Q: Is prepared by dissolving a definite weight of a substance in a definite volume. a. primary…
A: During the experiments, a standard solution is made to carry out the reaction and know the amount of…
Q: The Kc for the reaction 2A (aq)=3 B (aq) is 0.085. What is Kc for the reaction 3 B (aq) = 2A (aq)?
A: Welcome to bartleby !
Q: It is required to analyse the metal from its ore sample. Manganese (Mn) present in the ore sample…
A: The mass of the ore sample is = 2.98 g The mass of the MnSO4 precipitate is = 0.19 g The percentage…
Q: 3) A mixture of 80.0 g of chromium (VI) oxide, Cr2O3, and 8.00 g of solid carbon, C, is used to…
A: Number of moles=Given massmolar massGiven mass of Cr2O3=80.0gmolar mass of Cr2O3=(52*2+16*3) g/mol…
Q: Write the net equation for precipitation of AgI when aqueous solutions of AgNO3 and Nal are mixed.…
A: AgNO3 react with NaI to give AgI.
Q: The Yucca Mountain repository in Nevada, which is intended for the long-term storage of nuclear…
A: Concept introduction- Solubility product (Ksp)- It is equilibrium constant for a chemical reaction…
Q: 3. A student investigated the stoichiometry of the reaction of zinc (Zn) with HCl solution and…
A: Density of a substance is given as,Density = Mass Volume
Q: Brass is an alloy consisting mainly of copper and zinc. To determine the percentage of copper in a…
A: The mass of the total sample of brass is given as 2.63 g. The amount of copper present in the sample…
Q: A student Investigated the stoichiometry of the reaction of zinc (Zn) and HCl solution and reported…
A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…
Q: We want to determine the purity of alum sample bought in a local pharmacy in Miagao. A Chem 28…
A: Mass of sample = 1.5879 gm Mass of Al2O3 = 0.1572 gm Molar mass of potash alum = 474.4 gm/mole…
Q: applications of precipitation in chemistry?
A: INTRODUCTION: Precipitation reaction is defined as the reaction in which precipitates form in…
Q: The titration of 25.0 mL of an iron(II) solution required 18.0 mL of a 0.115 M solution of…
A: Net ionic equation for the reaction between iron(II) and dichromate is shown below. Number of moles…
Q: A chemist adds 0.30 L of a 2.04M sodium thiosulfate (Na, S,0,) solution to a reaction flask.…
A:
Q: Write a balanced chemical equation describing the mixing of the following 2 reagents in aqueous…
A:
Q: To determine the amount of magnetite, Fe3O4, in an impure ore, a 1.5419-g sample is dissolved in…
A:
Q: "Native," or elemental copper can be found in nature, but most copper is mined as oxide or sulfide…
A: Given , 1 penny contains mass of copper= 3.000 g
Q: The amount of calcium carbonate (CaCO3; molar mass = 100.1 g mol-1) in the ore dolomite can be…
A: Theoretical yield of the product is given by: Theoretical yield of the product = Molecular mass…
Q: The aluminium in a 1.2 g sample of impure NH4Al (SO4)2 was precipitated as hydrous Al2O3. The…
A: The number of moles is defined as the ratio of the mass of a substance to its molar mass. Number of…
Q: 1,5419 g of magnetite (Fe3O4) ore; in concentrated HCL to form a mixture of Fe + 2 and Fe+3 it's…
A:
Q: Consider the reaction between ammonium dichromate and iron (III) acetate which occurs by the…
A: Molarity is the unit of concentration of a solution, and its unit is mol/L. It is defined by the…
Q: The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitated with aqueous…
A: Mass of Sample is 1.200 g. Mass of anhydrous Al2O3 is 0.2001 g. Calculation of no. of mol of…
Q: KMnO4 according to the following chemical equation: K2C2O4 (aq) + 2 KMnO4 (aq) + 8 H2O →10 CO2…
A: Based on the balanced chemical equation for the given reaction and following simple unitry method we…
Q: 10. An ore containing magnetite, Fe304, was analyzed by dissolving a 0.9859-g sample in concentrated…
A: Answer: This question is based on stoichiometric calculation where we have find out the number of…
Q: Write the chemical reaction of Iron Sulfide (FeS2) to create Sulfuric acid in mines. It reacts with…
A: It is used in the preparation of hydrogen sulphide gas.In hair dyes, paint, ceramics, bottles and…
Q: Solution A was prepared by weighing 6.08 grams of K3Fe(CN)6 (MW 329.2 g/mol) and dissolving the…
A: Given the mass of K3Fe(CN)6 taken to prepare the solution-A = 6.08 g Molar mass of K3Fe(CN)6 =…
Q: You are told by your instructor to go to the stock room and find a bottle of the chemical K3Cl. Does…
A: Given formula of chemical is K3Cl We need find whether a compound with this formula exist or not
Q: What is the significance of adding sodium fluoride in the test solution in the analysis of cobalt…
A: In analysis of cobalt ion sodium fluoride is added
Q: Adult oyster shells are composed mainly of calcite, CaCO3. It’s dissolution in water can be…
A:
Q: The Kc for the reaction 2A (aq) ⇌ 3 B (aq) is 0.085. What is Kc for the reaction 3 B (aq) ⇌ 2A (aq)?
A: Characteristics of Kc : If reverse the equilibrium reaction, Kc value is reciprocated. In the given…
Q: 4 Define the following symbols: a. S d. G b. AS e. AG с. Т
A:
Q: In the laboratory you are given the task of separating Ag* and Fe2+ ions in aqueous solution. For…
A: Answer-1 No, by the use of K2CO3 it is not possible to separate silver ion and ferrous ion because…
Q: A chemistry student is doing a titration lab and needs to make up 2 liters of NaOH for the class and…
A: Titration is the method finding the strength of the unknown solution with the help of unknown…
Q: Solution A was prepared by weighing 6.08 grams of K3Fe(CN)6 (MW 329.2 g/mol) and dissolving the…
A:
Q: A substance which cannot be broken down by distillation, electrolysis or heating is most likely c. a…
A: elemental substance is the class of pure substance that can not be separated in to two or more…
Q: Hydrogen peroxide solutions can casily be decomposed by dust, trace amounts of metals or light. It…
A: Given: Density of hydrogen peroxide solution = 1.11 g cm-3 = 1.11 g/mL Volume of H2O2 used for…
Q: "Native," or elemental copper can be found in nature, but most copper is mined as oxide or sulfide…
A: (a) As specified by the question - one copper penny has a mass of 3g. therefore, 100 copper penny…
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
- By pipet, 15.00ml of the stock solution of potassium permanganate (KMn04) that was prepared by dissolving 13.0g KMn04 with DI H20 in a 100.00ml volumetric flask, diluting to the calibration mark was then transferred to a 50.00ml volumetric flask and diluted to the calibration mark. Determine the molarity of the resulting solution.In the laboratory, a student was tasked to prepare a stock solution of HCl for titration. The available analytical grade HCl solution in the stock room was labelled 35% w/v HCl. The student proceeded to prepare the stock solution by mixing 10mL of the HCl solution with 490mL of analytical grade water. Then, the solution was further diluted by adding 5mL, since the total volume of the solution did not reach the 500mL etched mark on the volumetric flask. To prepare the titrant, the student mixed 10mL of the stock solution, then added 40mL of analytical grade water. The titrant was subsequently used to determine the concentration of two titrand. *Use the table as a reference 1. What is the normality of the available HCl reagent in the stock room?* 5.08 N 10.15 N 20.3 N 11.0 N None of the choices 2. What is the normality of the stock solution of HCl?* 0.09N 0.10N 0.11N 0.12N None of the choices 3. What is the normality of the titrant?*…A 25.00mL wastewater sample was analyzed for its Mg2+ content using a standard gravimetric method. the sample was diluted to 3.00L and an 11.00mL aliquot was treated to precipitate magnesium as MgNH4PO4.6H2O using (NH4)2HPO4 as the precipitating agent. the precipitate was then filtered, washed, dried, and ignited resulting in a 0.1325mg Mg2P2O7 residue. How much Mg (in ppm) is present in the original sample
- In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) Question: Is the reaction balanced?In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) Is the reaction balanced? What was in the bubbles? What were the actual, theoretical, and percent yields of sodium chloride (NaCl)? You must show your work to receive credit.In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) What were the actual, theoretical, and percent yields of sodium chloride (NaCl)?
- In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) Question: What were the actual, theoretical, and percent yields of sodium chloride (NaCl)?A sample containing chlorophenol, C6H4ClOH, was analysed by gravimetric analysis. A 0.783-g of this sample goes through a chemical process allowing the chlorine in the chlorophenol to precipitate as silver chloride, weighing 0.271 g. Calculate the % (wt/wt) of the chlorophenol in the sample, assuming that chlorophenol is the only source of chlorine in the sample. Provide your answer to two decimal places and without units. Avoid using scientific notation.Drug: C20H22ClN (Flexeril also known as iCyclobenzaprine HCl Using unit analysis, clearly show the set-ups for your calculations. You wish to prepare 50.0 mL of 2.30 x 10–2 M solution of your drug. (hint-how many grams will you need of your drug?) Describe how to prepare this solution from the pure drug and deionized water. Analytical balances and volumetric flasks are available to you. (Assume that your drug dissolves in water, at least to the extent necessary for this problem.) Use complete sentences in your description of the solution preparation process. A patient is given 2.0mL of a 3.00% (m/v) solution of your drug, how many milligrams of the drug did they receive? What is the molarity of a 3.00% (m/v) solution of your drug?
- A stock solution of potassium permanganate (KMn04) was prepared by dissolving 13.0g KMn04 with DI in a 100ml volumetric flask and diluting to the calibration mark. Determine the molarity of the solution.A sulfuric acid spill occurred on the highway after a truck containing barrels of sulfuric acid swerved out of control from a truck tire blowout. Luckily no one got hurt in the event but there is a concern that the sulfuric acid spill may affect local ground water supply. A sample of the ground water in that area was recovered to assess the extent of contamination of the ground water supply. In order to determine the concentration of sulfuric acid in the sample, 25.00 mL of the ground water sample was titrated with 0.133 M NaOH and you get the following data: Sodium hydroxide (initial buret reading) 0.66 mL Sodium hydroxide (final buret reading) 17.42 mL Calculate the molarity of sulfuric acid in the ground water sample. Enter numerical answer. Report in 3 sig figs. Show work6. A stock solution containing 25% w/v of chlorhexidine is used to prepare an antiseptic such that when the antiseptic is diluted 1 in 25, a 1 in 500 wash solution is obtained which is ready for use by the patient. What volume (ml) of the stock solution is required to prepare 5 litres of the antiseptic to fulfil a bulk manufacturing order?