Lab Report 4 Dearing

Based on this student data, calculate the average molarity of the NaOH solution. Standard: KHP = potassium hydrogen phthalate, MM 204.4 g/mol Student Data Trial 1 E KHP mL initial: NaOH mL final: NaOH 2.02 0.57 19.25 Trial 2 2.05 19.25 39.80 Trial 3 1.99 1.65 20.75

3) Propagation of uncertainty. Every measurement has uncertainty. In this problem, we'll evaluate the uncertainty in every step of a titration of potassium hydrogen phthalate (a common acid used in titrations, abbreviated KHP, formula CsH5KO4) with NaOH of an unknown concentration. The calculation that ultimately needs to be carried out is: concentration NaOH 1000 x mass KHP × purity KHP molar mass KHP x volume NaOH Measurements: a) You use a balance to weigh 0.3992 g of KHP. The uncertainty is ±0.15 mg (0.00015 g). b) You use a buret to slowly add NaOH to the KHP until it reaches the endpoint. It takes 18.73 mL of NaOH. The uncertainty of the burst is 0.03 mL.. c) The manufacturer states the purity of KHP is 100%±0.05%. d) Even though we don't think much about them, molar masses have uncertainty as well. The uncertainty comes from the distribution of isotopes, rather than random measurement error. The uncertainty in the elements composing KHP are: a. Carbon: b. Hydrogen: ±0.0008…

Ca2+ in a drinking water sample was analyzed by the following reactions below: Ca2+(aq) + C2O42-(aq) → CaC2O4 (s) → CaO(s) + CO(g)+ CO2(g) First an excess of C2O42- was added to 0.10 L of the Ca2+ water sample. Then CaC2O4 was precipitated, which was demcomposed into CaO with filtering and some heat. The CaO was measured to be 5.61 mg. What is the concentration of Ca2+ in the original water sample? The MW of CaO is 56.1 g/mol.      0.0100M     0.0010 M     1.00 M     0.100 M   The partition coefficient (K) of methylamine (CH3NH2) is 4.50, preferring the organic layer over the aqueous layer in this extraction. The Ka of methylammonium (CH3NH3+) is 2.00 x 10-11. If 10 mL aqueous methylamine solution at pH 11.0 is extracted with 20.0 mL organic solvent, what is the fraction of solute remaining in the water (q)?   HINT: methylamine is a weak base.     14.3%     10.0%     18.2%     81.8%

Analytical chemistry

A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.

K2CO3 (aq)+ CaCl2 (aq)→ CaCO3 (s) + 2KCl (aq)   Data Sheet Table 1: Data and Observations Material  Mass CaCl2  2.0g K2CO3  2.5g Filter Paper 1.6g Watch Glass 35.8g Filter Paper + Watch Glass + Precipitate 38.9 Precipitate 1.5g   Table 2: Mass of CaCl2 after 24 Hours   Initial Observations 24 hour Observation Weigh Boat Mass of Weigh Boat 0.5g Mass of Weigh Boat 0.5g CaCl2 2.0g  Mass of CaCl2  2.4g Mass of CaCl2    Calculate the theoretical yield of the solid precipitate. Then use that to calculate the percent yield of the solid precipitate.

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3-6 3 SOLUTIONS AND NAME SOLUTION CONCENTRATIONS 1415 Section Pre-Lab Assignment Experiment objectives A, B, and C require you to devise procedures for preparing a saturated aqueous solution of potassium sulfate, experimentally determining the density of this solution, and experimentally determining the mass percent of potassium sulfate in this solution. Your pre-lab assignment is to develop procedures for parts A, B, and C. You will then execute these procedures in lab. PREPARATION OF A SATURATED AQUEOUS POTASSIUM SULFATE SOLUTION Reminder: use a maximum of 75 mL of water. A. В. DENSITY OF SATURATED AQUEOUS POTASSIUM SULFATE SOLUTION C. MASS PERCENT OF POTASSIUM SULFATE IN A SATURATED POTASSIUM SULFATE SOLUTION

What are the Volumes of HCl from the 3 Trials?

can be used as a standard solution for checking the concentration of a solution containing sulphuric acid, 8.7 cm' of sulphuric acid. Find the concentration of the sulphuric acid in both mol dm3 and g dm³. In a particular experiment 10,0 cm³ of a 0.50 mol dm³ solution of sodium ethanedioate was found to react with Q2. Sodium ethanedioate, Na;C¿O4, can be made into a solution of an exact and reliable concentration and so London ndon A.C.1.2

Complete the balanced molecular reaction for the following weak acid with a strong base. Be sure to include the proper phases for all species within the reaction. 1 + 2 Ca HNO₂(aq) + Ca(OH)₂ (aq) 3 H ²- 4 -> OH 5 = 6 H3O+ 6 (s) 7 H₂O 3+ 8 4+ N 9 0 (1) (g) (aq) O o

The first goal is to make the oxalic acid standard solution.  You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL.   Molar mass of H2C2O4•2H2O = 126.07 g/mol   Mass of H2C2O4•2H2O = 1.5232g what is the Number of moles of H2C2O4•2H2O?

The first goal is to make the oxalic acid standard solution.  You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL.   Molar mass of H2C2O4•2H2O = 126.07 g/mol   Mass of H2C2O4•2H2O = 1.5232g  Volume of H2C2O4•2H2O  solution = 250.0mL    What is the Molarity H2C2O4 standard solution ?

During a lab on qualitative analysis, an unknown solution containing one cation was analyzed and the following data was collected: Anions Added to the Unknown Solution S²- SO4²- OH CO3²- Which one of the following cations is found in the unknown solution? CATIONS Ba2+ Ca²+ Sr²+ High Solubility (aq) Observation Be2+ Mg2+ no precipitate precipitate precipitate precipitate Cl, Br, I- Halides Ag+, Pb²+, Low Solubility Tl+, Hg₂²+, (s) Hg, Cu Most S2- Solubility Table Group 1, NHÀ, Group 2 Most ANIONS OH Group 1, NH4*, Sr²+, Ba²+, Tl Most SO4²- Most Ag+, Pb²+, Ca²+, Ba²+, Sr²+, Ra²+ All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. CO3²-, C₂H3O2 NO3 PO4³-, SO3²- Group 1, Most All NH4* Most Ag+ None

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Questions 30 and 34. The correct answers are in pink

What is the purity test of salicylic acid and commercial aspirin?

Complete the balanced neutralization equation for the reaction below. Be sure to include the proper phases for all species within the reaction. П + Reset 0₂ C 1 2 3 4 HC₂H₂O₂(aq) + Sr(OH)₂(aq) 2 3 2 3 ■ U 00 Question 52 of 70 ■ O LO 5 6 + ☐6 ²+ 3+ 2+ 7 8 9 07 ☐8 H 4+ U 0 (s) (1) (g) (aq) Sr 口。 • x H₂O Delete Submit +

In the analysis of H2O2 using KMnO4, the simulation first states that about 20 mL of water is added to the 1.00 mL aliquot of H2O2 to make the observation of the end point easier. Later, you are informed that your assistant diluted the 1.00 mL H2O2 sample to 10 mL with distilled water. Which of the following volumes is used in your analysis of the concentration of H2O2 in the original sample? Question 3 options: 10.00mL 20.00mL 11.00mL 21.00mL  1.00mL

A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O.   a.Write the ionic equation for the reaction.   b.Write the net ionic equation for the reaction.   c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture?   d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture?   e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)?   f.What is the percent by mass of each salt in the mixture

The aluminum in a 2.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous ‍‍Al2O3⋅xH2O. The precipitate was filtered and ignited at 1000°C to give anhydrous Al2O3, which weighed 0.3006 g. Express the result of this analysis in terms of a. %NH4Al(SO4)2 b. %Al2O3 c. %Al

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.

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7 Solid lead (II) nitrate is slowly added to 125 mL of a 0.190 M potassium hydroxide solution until the concentration of lead ion is 0.0547 M. The percent of hydroxide ion remaining in solution is %. Submit Answer $ 4 R LLO % 5 [Review Topics) [References Use the References to access important values if needed for this question. Retry Entire Group T Cengage Learning | Cengage Technical Support ^ 6 * 8 more group attempts remaining MacBook Pro G H 2 & 7 A J * 0 8 ( 9 UD U K F 0 ) O ◆ P | Previous Email Instructor { [ + 11 = Next> Save and Exit } ]

Part A) A 10.0 mL sample of 0.250 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0900 mol/L NaOH(aq) and then diluted to a final volume of 100. mL.Calculate the concentration of Ni2+ ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.ksp: 5.48e-16