Q: The digestion of a 0.1387-g sample of a phosphorus containing compound in a mixture of HNO, and…
A: Solution: Given: Mass of the sample containing phosphorus = 0.1387 gMolarity of NaOH solution =…
Q: What is the pH when 25% of the acid H3AsO4 (pKa = 2.22) has reacted with NaOH in a titration?
A: The reaction of H3AsO4 with NaOH results in the conversion of 25% of the acid into its conjugate…
Q: 2. A solution that may contain Cu, Bi?", Sn*, or Sb* is treated with thioacetamide in an acidic…
A: 2. subjective examination Dark encourage halfway disintegrated in basic medium : could be Cu2+…
Q: A group of students were able to isolate a novel amylase from the saliva of a pig found in Country…
A: Given the desired pH = 7.4 We can find the most suitable buffer based on the Henderson equation.
Q: 2. A solution that may contain Cu", Bi?", Sn, or Sb?* is treated with thioacetamide in an acidic…
A: 1) A solution that may contain Cu2+, Bi2+, Sn4+, or Sb2+ is treated with thioacetamide in an…
Q: 2.4414 g sample containing KCl, K2SO4 and inert materials was dissolved in sufficient water to give…
A: Mohr method is the method to determine the chloride ion concentration of a solution. This is done by…
Q: For breakfast, the nihilistic Rick Sanchez ate 100 g of cereal mixed with 20 g of milk. A 1.500 g…
A: Given: The molar mass of N (nitrogen) is 14.07 g/mol. For cereal: The amount of cereal consumed is…
Q: Rewrite the reaction using chemical formulas and showing the states of matter (s, 1, g, aq) for the…
A: In the asked reaction HBr acts as an acid and water acts as a base. HBr donates a proton (H+) which…
Q: 2.4414 g sample containing KCl, K2SO4and inert materials was dissolved in sufficient water to give…
A: Given: Mass of sample = 2.4414 g. This sample contains KCl, K2SO4 and inert materials. The volume of…
Q: An organic acid has been added to a solution with an alkalinity of 50 mg/L of CaCo3. The alkalinity…
A: A numerical problem based on equilibrium concept, which is to be accomplished.
Q: what precipitate is formed in the reaction (CdBr2) and (Na2S)
A: Precipitation reaction : Durin this reaction, aqueous solution of two compounds mix to form an…
Q: .A sample of alfalfa meal weighing 2.0 g is analyzed by Kjeldahl method for the percentage of…
A:
Q: A 1.7483-g sample containing Al(NO3)3, AlCl3, and inert material was dissolved in acid and divided…
A:
Q: 5.31e-08 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 9.14e-08 g of…
A:
Q: 2.4414 g sample containing KCl, K2SO4and inert materials was dissolved in sufficient water to give…
A: Mohr method is the method to determine the chloride ion concentration of a solution. This is done by…
Q: Cl- is precipitated by addition of AgNO3?
A: Given Cl- is precipitated by addition of AgNO3?
Q: Cerium. 2. Why is it not advisable to dissolve KMnO4 in conc. H₂SO4?
A:
Q: What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9?…
A:
Q: Using the concentrations 0.100M and 0.1766M, and the pKa of 3.752, what is the theoretical pH of a…
A: pKa = 3.752
Q: A 0.951-g sample containing (NH4)2C2O4 and compounds was dissolved in water and made alkaline with…
A:
Q: Explain briefly in 2 sentences andin your OWN words. 1. NH4CNS used in the test for cobalt must be…
A: Gravimetric analysis is one of the most accurate analytical methods available. It is concerned with…
Q: Which compound, FeCO3 or PbBr2, is more soluble in acid than in base? Why?
A: The two given compounds are FeCO3 and PbBr2 . From the two given compounds, FeCO3 is more soluble in…
Q: A sample of water at pH 10.5 has 75 mg/L of CO3-2 and 65 mg/L of HCO3- Including the contribution of…
A:
Q: Calculate the pH at which pilocarpine (basic drug) starts to precipitate from a 2% w/v aqueous…
A: Solution- poOH=pKb + logConjugated acidbasegivehn pKa of pilocarpine…
Q: HCI, a strong acid, was added to a solution containing 2.67 g until the pyridine was 78% in its…
A: Buffer solution: It is a special type of mixture of a weak acid or a weak base and its conjugate…
Q: What is the K value for the acid base reaction of nitrous acid with sodium cyanide?
A: The equilibrium constant (K): The equilibrium constant (K) is the ratio of the concentrations of…
Q: Write the equilibrium constant expressions for the following chemical reactions (using the net ionic…
A:
Q: A pink solid has the formula CoCl3·5NH3·H2O. A solution of this solid is also pink in color and when…
A: given pink solid CoCl3·5NH3·H2O titration with 3 mol of AgCl. purple solid is formed
Q: A 1.219-g containing (NH4)2SO4, NH4NO3, and nonreactive substances was diluted to 200 mL in a…
A: Given: For the first titration, Mass of the given sample = 1.219g Volume of the sample = 200 mL…
Q: Sodium acetate, CH3COONa was hydrolysed in water, H2O. Show the reaction equations involved. What is…
A: Sodium acetate hydrolysis in water and formed acid and base.
Q: A sample of meat scrap weighing 2.000 g is digested with concentrated sulfuric acid and a catalyst.…
A: The answer is given below
Q: What is the value of pH for the soultion of CH3COOH and NH3 and why? In other words, in tittration…
A: An acid-base indicator (e.g., phenolphthalein) changes color depending on the pH. Redox indicators…
Q: Why is the equilibrium between the acid NaH2PO4, and its conjugate base Na2HPO4, a suitable buffer…
A: When a solution is referred to as a weak acid or weak base, it means that the solution can undergo…
Q: A 1.43 x 10-4 L solution of 45.7 mg/mL protein was analyzed using the Kjeldahl procedure. After…
A: Kjeldahl method is used to quantitative method and it is used in the determination of Nitrogen in…
Q: To find the percentage of Na2CO3 in the (Nacl + Na2CO3) mixture in a laboratory experiment…
A: Introduction: The reaction of sodium carbonate with hydrochloride acid has proceeded as given below.…
Q: When treated wi th a solution of ammonium sulfate, an un known solution gave no precipitate. A white…
A: We have to identify the ions present in the unknown solution out of the following :
Q: What do the ions that gave a precipitate when mixed with AgNO3 have in common?
A: Since the halogen ions react with Ag+ ions to form a precipitate Hence any anion whose salt with…
Q: Sulfuric acid (H2SO4) is a diprotic acid where the first deprotonation is a strong acid process, and…
A: Given, Molar concentration of H2SO4 = 0.00075 M Sulfuric acid (H2SO4) is a diprotic acid where the…
Q: If a sample of silver coin weighing 0.5230 g gives a precipitate of AgCl (143.45) weighing 0.3559 g,…
A: The mass of the silver coin sample is = 0.5230 g The mass of the AgCl precipitate is = 0.3559 g The…
Q: For breakfast, the nihilistic Rick Sanchez ate 100 g of cereal mixed with 20 g of milk. A 1.500 g…
A:
Q: What is the pH when preparing a solution od 1 mol NaOH and 2 mol of solid NaH2PO4? The pKa's of…
A: Given: Moles of NaOH = 1 mol. Moles of NaH2PO4 = 2 mol.
Q: A 0.5843-g sample of a plant food preparation was analyzed for its N content by the Kjeldahl method,…
A:
Q: To rule out metabolic acidosis in a patient's blood sample, the total carbon dioxide content should…
A: Henderson-Hasselbach equation. this equation shows the relationship between pH of a solution, the…
Q: 2. In an iodometry titration, the appearance of blue colour upon addition of starch indicator is…
A: Iodometry titration can be defined as a method of volumetric analysis where the appearance or…
Q: a mixture of compounds was dissolved in organic solvent and extracted with NaOh. The NaOH extract…
A: Phenols and carboxylic acid react with NaOH forms corresponding salts. These salts are soluble in…
Q: Calculate the pK, of hypobromous acid from its K, value.
A: Since you have posted multiple questions, we are entitled to answer the first only.
Q: A sample of alfalfa meal weighing 2.0 g is analyzed by Kjeldahl method for the percentage of…
A: Kjeldahl analysis is used for the quantitative determination of N in protein and other samples.
Q: H.W 1) Calculate the number of meq. of H;C:0.2H;0 (fw= 126.1) in 0.5 gm of the pure compound…
A:
Q: Sulfur containing compound weighing 4.8670 grams was digested and purified to form H,SO4. A 25.00-mL…
A: Moles = Molarity * Volume (L) Mass = Moles * Molar mass
When H2SO4(aq) was reacted with NaOH(aq) in the titration, why was a precipitate not formed?
Step by step
Solved in 2 steps
- Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+H2O(l)An aqueous solution of Ca(OH)2with a concentration of 0.209 M was used to titrate 25.00 mL of aqueous HCl. 15.93 mL of the Ca(OH)2was required to reach the endpoint of the titration. A. How many moles of base were required to react completely with the acid in this reaction? _____mol Ca(OH)2 B. How many moles of HCl were present in the original 25.00 mL of acid?______mol HClA solution contains S 2– and SO 42– ions. In what order dowe add Ag(NO 3 )(aq) and Ba(NO 3) 2(aq) to separate eachanion independently? Which precipitates form?What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9? The pK a of the acid is 5.7.
- 25 g of the dilute mixture of H2SO4 and HNO3 is completed to 500 mL with water. When BaCl2 is added to 10 mL of this solution, the precipitate obtained is 362 mg. Another 20 mL portion taken from the solution is neutralized with 39.2 mL of 0.2 M NaOH solution in the presence of phenolphthalein. Calculate the percentage of HNO3 in the starting mixture.A 0.4126-g sample of primary-standard Na2CO3 was treated with 40.00 mL of dilute perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back - titrated with 9.20 mL of dilute NaOH. In a separate experiment, it was established that 26.93 mL of the HClO4 neutralized the NaOH in a 25.00-mL portion. Calculate the molarities of the HClO4 and NaOH.Given that Ksp for AgCl is 1.6E-10 and Kf for Ag(CN)2- is 5.6E8, calculate the concentration of Ag+ when 0.15 M AgNO3 is reacted with 0.25 M KCN.
- A 0.4126-g sample of primary-standard Na₂CO₃ was treated with 40.00 mL of dilute perchloric acid. The solution was boiled to remove CO₂, following which the excess HClO₄ was back-titrated with 9.20 mL of dilute NaOH. In a separate experiment, it was established that 26.93 mL of the HClO₄ neutralized the NaOH in a 25.00-mL portion. Calculate the molarities of the HClO₄ and NaOH. Input your answer in compound form (i.e. x.xx M HClO4 and x.xx M NaOH) with the correct significant figures.The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 20.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH. After cooling, the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2SO4. Calculate the amount of ethyl acetate (88.11 g/mol) in the original sample in grams.5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)
- (a) Sodium acetate, CH3COONA was hydrolysed in water, H2O. Show the reaction equations involved. What is the effect of the salt on the pH of this solution? (b) (i) Define buffer solution. (ii) 2.50 g of sodium acetate, CH3COONA was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M ethanoic acid, CH3COOH was added into the above salt solution. Calculate the pH of the mixed solution. [pKa of CH3COOH = 4.75, Molar mass of CH3COONA = 82.0 g mol-1] (c) Explain how the above buffer solution maintain its pH when a small amount of sodium hydroxide, NaOH is added.1. When H2SO4(aq) was reacted with NaOH(aq) in the titration, why was a precipitate not formed? 2. Why did the colour of the solution in the conical flask change at the end of the titration? 3. In this acid-base titration, what did we use to measure the volume of the H2SO4(aq)? 4. What do we mean by stoichiometric point of a titration?A 1.00 L phosphate buffer solution that contains 0.1270 moles of dihydrogen phosphate (H2PO4) and 0.0800 moles of hydrogen phosphate (HPO,2-) was prepared. The pKa of dihydrogen phosphate is 7.20 at 25 °C. Calculate the pH of the buffer at this temperature.