QUESTION 4Mg(OH)2 reacted with dilute hydrochloric acid as following equation.Mg(OH)2(s) + 2HCI(aq) -MgCl2(aq) + 2H20(mCalculate the mass of excess reagent remaining at the end of the reaction when 27.63 mL of 0.5 M HCIwere reacted with 500 mg of Mg(OH)2-QUESTION SDuring titration, the following data were collected. A 50.0 mL portion of an HCI solution was titrated with 0.500 MNaOH, 200. ml of the base was required to neutralize the sample. How many grams of HCI are present in 89 mlof this acid solution?QUESTION 6Phosphorus pentachloride (PCls) reacts with water to form hydrochloric acid (HCI) and phosphoricacid (H3PO4). How many total moles of acids are formed when starting with 51.98 g of PCI5 and excessH2O?PCIS + 4H20 - SHCI + H3PO4

Given, Mg(OH)2(s) + 2HCl(aq) → MgCl2(aq) + 2H2O(l) concentration of HCl solution = 0.5 M = 0.5 mol/L…

QUESTION 4 MgtOH)2 reacted with dilute hydrochloric acid as following equation. Mg(OH)2(s) + 2HCI{aq)MgCl2(aq) + ZH20(1) Calculate the mass of excess reagent remaining at the end of the reaction when 27.63 ml of 0.5 M HCI were reacted with 500 mg of Mg(OH)2-

QUESTION 4 MgtOH)2 reacted with dilute hydrochloric acid as following equation. Mg(OH)2(s) + 2HCI{aq)MgCl2(aq) + ZH20(1) Calculate the mass of excess reagent remaining at the end of the reaction when 27.63 ml of 0.5 M HCI were reacted with 500 mg of Mg(OH)2-

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 37QAP: An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is...

See similar textbooks

Similar questions

A student is given 0.930 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.615 M NaOH. The equivalence point is reached when 33.6 mL are added. What is the unknown acid?
95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?
Calcium ions in blood trigger clotting. To prevent that in donated blood, sodium oxalate, Na2C2O4, is added to remove calcium ions according to the following equation. C2O42(aq)+Ca2+(aq)CaC2O4(s)Blood contains about 0.10 mg Ca2+/mL. If a 250.0-mL sample of donated blood is treated with an equal volume of 0.160 M Na2C2O4, estimate [Ca2+] after precipitation. (KspCaC2O4=4109)
Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel. It can be prepared in the general chemistry laboratory by treating nickel(II) acetate with formic acid (HCO2H). Ni(CH3CO2)2(aq) + 2 HCO2H(aq) Ni(HCO2)2(aq) + 2 CH3CO2H(aq) Green crystalline Ni(HCO2)2 is precipitated after adding ethanol to the solution. (a) What is the theoretical yield of nickel(II) formate from 0.500 g of nickel(II) acetate and excess formic acid? (b) Is nickel(II) formate paramagnetic or diamagnetic? If it is paramagnetic, how many unpaired electrons would you expect? (c) If nickel(II) formate is heated to 300 C in the absence of air for 30 minutes, the salt decomposes to form pure nickel powder. What mass of nickel powder should be produced by heating 253 mg of nickel(II) formate? Are nickel atoms paramagnetic?
A solution of tartaric acid(H₂C₄H₄O₆)with known concentration of 0.155 M H₂C₄H₄O₆ is titrated with a 0.425 M NaOH solution.How many mL of NaOH are required to reach the second equivalence point with a starting volume of 70.0 mL H₂C₄H₄O₆ ,according to the following balanced chemical equation : H₂C₄H₄O₆+ 2 NaOH→Na₂C₄H₄O₆+ 2 H₂O
A 20.00-mL sample of aqueous oxalic acid, H2C2O4, was titrated with a 0.09113-M solution of potassium permanganate, KMnO4. A volume of 23.24 mL was required to reach the endpoint. What is the molarity of oxalic acid?
A solution of citric acid (H₃C₆H₅O₇) with a known concentration of 0.200 M H₃C₆H₅O₇ is titrated with a 0.750 M NaOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 25.0 mL H₃C₆H₅O₇ , according to the following balanced chemical equation: H₃C₆H₅O₇ + 3 NaOH → Na₃C₆H₅O₇ + 3 H₂O
A student weights out 1.118g of impure KHP, dissolves the sample in deionized water and titrate it with 0.1001 M NaOH solution. If the titration requires 27.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?
Conducting a titration Your objective is to determine the concentration of a solution of acid HA by means of an acid-base titration, using a 0.15 M solution of the base B(OH)2 and methyl orange as indicator. The unbalanced reaction between HA and B(OH)2 is shown below. Figure 3 shows the experimental set-up: the analyte was 20 mL of 0.15 M B(OH)2, and the titrant was the solution of HA of unknown concentration. B(OH)2 + HA → BA2 + H2O Materials provided a solution of HA of unknown molarity (titrant) a solution of B(OH)2 of concentration 0.15 M (analyte) methyl orange indicator Equipment per station Stand, clamp, white tile conical flask (100 mL) Burette (50 mL) Pipette (25 mL) Glass funnel Paper towels, pasteur pipettes, pen (for labelling glassware), beaker a) Using Figure 3 and the equipment and materials lists provided, outline how you would carry out a series of titrations to determine the molarity of the HA solution (Wordcount: 250 words). b) The starting and end…
1. 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. 2. A 0.5002-g sample that assayed 96.4% Na2SO4 required 48.63 mL of a barium chloride solution. Reaction: Ba2+ + SO42+ → Ba SO4 (s) Calculate the analytical molar concentration of BaCl2 in the solution. 3. A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate: (a) the molar analytical concentration of K3Fe(CN)6. (b) the molar concentration of K+. Using step-by-step process
In the titration of acetic acid, CH3COOH, a 0.20 M solution of NaOH is used. A volume of 15.00 mL of CH3COOH solution istitrated. If it takes a total of 24.55 mL of NaOH solution to reach the equivalence point, what is the molar concentration of theCH3COOH solution?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 115. mg of oxalic acid (H2C2O4). a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxallc acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 76.4 ml of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution, Be sure your answer has the correct number of significant digits.