Calculate the concentration of the hydrochloric acid if a 20.00 mL sample is titrated with standard sodium carbonate solution. 2 HCl (aq) + Na2CO3 (aq) → H2O (l) + CO2 (g) + 2 NaCl (aq) The titration required 10.00 mL of 0.250 mol/L sodium carbonate to neutralize the acid.

Calculate the number of milliliters of 0.587 M KOH required to precipitate all of the Mg²+ ions in 102 mL of 0.753 M MgCl₂ solution as Mg(OH)2. The equation for the reaction is: MgCl₂ (aq) + 2KOH(aq) → Mg(OH)2 (s) + 2KCl(aq) Volume = mL

W Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed. O 2 H* (aq) + CO3²-(aq) → H₂CO3(s) 2 Na* (aq) + CO3²- (aq) + 2 H*(aq) + 2 Cï(aq) → H₂CO3(s) + 2 NaCl(aq) O 2 H* (aq) + CO3²-(aq) → H₂O(1) + CO₂(g) 2 Na* (aq) + CO3²- (aq) + 2 H* (aq) + 2 Cl(aq) → H₂CO3(s) + 2 Na*(aq) + 2 Cl(aq) No reaction occurs.

You have been provided with a 2.08 x 10-2 L  sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?

Titration is a common laboratory method of quantitative chemical analysis. In an acid- base titration, 65.0 mL of Ba(OH)2 was neutralized by 58.0 mL of 0.350 mol/L HCl. Calculate the concentration of Ba(OH)

An analytical chemist weighs out 0.181 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 15.9 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. ol. g mol Ar

To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.3600M silver nitrate AgNO3 solution to a 24.00g sample of the fluid and collects the solid silver chloride AgCl product. When no more  AgCl is produced, he filters, washes and weighs it, and finds that 1.28g has been produced. The balanced chemical equation for the reaction is: Cl−(aq) + AgNO3(aq) -> AgCl(s) + NO−3(aq) What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Cl in the sample. Be sure your answer has the correct number of significant digits.

Calculate the number of milliliters of 0.479 M Ba(OH)2 required to precipitate all of the Cr³+ ions in 156 mL of 0.725 M CrIs solution as Cr(OH)3. The equation for the reaction is: 2Crls (aq) + 3Ba(OH)2 (aq) → 2Cr(OH)s (8) + 3Bal, (aq) ml. Volume= Submit Answer Retry Entire Group 9 more group attempts remaining

Jake carried out three titrations to determine the concentration of unknown nitric acid (HNO3) using 0.1050 M NaOH. He titrated 100.0 mL of the nitric acid sample and obtained the following volumes of NaOH: 20.56, 20.48, and 20.52 mL. The acid-base reaction occurring is NaOH (aq) + HNO3(aq) →→ NaNO3(aq) + H2O(l) Determine the concentration of the acid; report the average molarity with standard deviation. Pay attention to the number of significant figures on the mean and the number of decimal places on the standard deviation.

Using solubility rules, predict which compound precipitates in the following reactions. Then balance the chemical equations, writing out the total-ionic equations and net-ionic equations. BaCl2(aq) + (NH4)2CO3(aq) → BaCO3(s) + 2NHẠCI(aq)