chem
- 👍
- 👎
- 👁
- ℹ️
- 🚩
-
- 👍
- 👎
- ℹ️
- 🚩
-
- 👍
- 👎
- ℹ️
- 🚩
-
- 👍
- 👎
- ℹ️
- 🚩
Respond to this Question
Similar Questions
-
Chemistry
A sample of impure magnesium was analyzed by allowing it to react with excess HCl solution: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) After 1.27 g of the impure metal was treated with 0.100 L of 0.768 M HCl, 0.0125 mol HCl remained. -
Chimestry
(Iron ore is impure Fe_2O_3. When Fe_2O_3 is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. From a sample of ore weighing 950kg , 533kg of pure iron is obtained). What is the mass -
Chemistry
A 0.879 g sample of a CaCl2 ∙ 2 H2O / K2C2O4 ∙ H2O solid salt mixture is dissolved in 150 mL of deionized water. A precipitate forms which is then filtered and dried. The mass of this precipitate is 0.284 g. The limiting -
chemestiry
Al2(SO4)3(aq) + BaCl2(aq) BaSO4(s) + AlCl3(aq) Consider the unbalanced equation above. A 0.680 g sample of impure Al2(SO4)3 reacts with excess BaCl2. If the sample produces 0.530 g of BaSO4, what is the mass percent of Al2(SO4)3
-
Chemistry
The piperazine content of an impure commercial material can be determined by precipitating and weighing the diacetate: (C2H4)2N2H2 + 2 CH3COOH → (C2H4)2N2H2(CH3COOH)2 In one experiment, 0.3126 gram of the sample was dissolved in -
Analytical chemistry
A 0.6334 gram of sample of impure mercury (II) oxide was dissolved in an unmeasured excess of potassium iodide. Reaction: HgO + 4I- + H2O ------→HgI42- + 2OH- Calculate the % HgO in the sample if titration of the liberated -
Chemistry
1.2048g sample of impure Na2CO3 is dissolved and allowed to react with a solution of CaCl2 resulting CaCO3 after precipitation, filtaration and drying was found to weight 1.0362g. calculate the percentage purity of Na2CO3 -
Chemistry
In the analysis of 0.8503 g of impure chloride containing sample, 1.250 g of AgCl were precipitated out. What is the percent of mass of chlorine in the sample. (FW of AgCl = 143.32 g/mol, FW of Cl =35.453)
-
Chemistry
A sample weighing 3.064 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96). When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The Al2O3 does not -
chemistry
CrCl3(s) + AgNO3 (aq)= AgCl(s) + Cr(NO3)3(aq) A 0.750 g sample of impure CrCl3 was removed from a bottle that contained 1.75 g of impure sample. The removed sample was dissolved in water and required 42.5 mL of 0.215 M AgNO3 -
AP chem
A 0.345g sample of anhydrous BeC2O4, which contains an inert impurity, was dissolved in a sufficient water to produce 100ml of solution. A 20.0ml portion of the solution was titrated w/ KMnO4(aq). The balanced equation for the -
Chemistry
A 0.450-gram sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is: CaCO3(s)+2HCl(aq) -> CaCl2(aq) + H2O(l) + CO2(g) The excess HCl(aq) is titrated by 9.75 mL of 0.125 M NaOH(aq).
Still need help? You can ask a new question.