chem

a sample containing bacl2.2h2o,kcl snd inert material weighed 0.8417g. after heating the sample at 160c for 45 minutes it weighed 0.8076g. the sample was then desolved in water and treated with the slight excess of agno3. the resulting precipitate was collected and found to weigh 0.5847g. calculate the % bacl2.2h2o and kcl in the sample

  1. 👍 0
  2. 👎 0
  3. 👁 259
  1. mass H2O driven off at 160 C = 0.8417 - 0.8076 = ?
    Convert grams H2O to mols. mols = g/molar mass = ?
    1/2 that = mols BaCl2.2H2O.
    Convert to grams BaCl2.2H2O. g = mols x molar mass = ?
    %BaCl2.2H2O = (g BaCl2.2H2O/mass sample)*100 = ?

    How much AgCl would we get from the BaCl2.2H2O? That's
    mass BaCl2.2H2O x (2*molar mass AgCl/molar mass BaCl2.2H2O) = ??
    0.5847 g AgCl total - g AgCl from BaCl2.2H2O = ? = mass AgCl from KCl.
    Convert mass AgCl from KCl to grams KCl. That's g AgCl x (molar mass KCl/molar mass AgCl) = ?
    Finally % KCl = (grams KCl/mass sample)*100 = ?
    Post your work if you get stuck.

    1. 👍 0
    2. 👎 0
  2. what is the mass sample

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. general chemistry

    a 5.95 g sample of AgNO3 is reacted with excess BaCl2 according to the equation 2AgNO3 + BaCl2 yields 2AgCl + Ba(NO3)2 to give 3.17 g of AgCl. What is the percent yield of AgCl?

  2. chemistry

    treatment of a 0.400g sample of impure potassium chloride with an excess of AgNO3 resulted in the formation of 0.733g of AgCl. calculate the percentage of KCl in the sample. show balanced equations in support of your answer

  3. Chemistry

    The formaldehyde content of a pesticide preparation was determined by weighing 0.3124g of the liquid sample into a flask containing 50.0mL of 0.0996M NaOH and 50mL of 3% H2O2. Upon heating, the following reaction took place: OH- +

  4. Chemistry

    A 0.700 g sample containing Ag2O and inert material is heated, causing the silver oxide to decompose according to the following equation: 2 Ag2O(s) → 4 Ag(s) + O2(g) If 13.8 mL of gas are collected over water at 27°C and 1.00

  1. Chemistry

    What will happen if a mixture of BaCl2.2h2O and KCl heated up to 150 centigrade ?

  2. Chemistry

    A 0.60 g sample consisting of only CaC2O4 & MgC2O4 is heated at 5000C, converting the two salts of CaCO3 and MgCO3 . The sample then weighs 0.465 g. If the sample had been heated to 9000C, where the products are CaO & MgO, what

  3. chemistry

    Consider a mixture of the two solids BaCl2 * 2H2O (FW=244.26 g/mol) and KCl (FW=74.551 g/mol). When the mixture is heated to 160 C for 1 hour, the water of crystallization is driven off: BaCl2 * 2 H2O (s)  BaCl2(s) + 2 H2O(g) A

  4. Chemistry

    Consider a mixture of the two solids BaCl2.2H2O (FM 244.26) and KCl (FM 74.551). When the mixture is heated to 160C for 1 hour, the water of crystallization is drive off: BaCl2.2H2O --> BaCl2(s) + 2H2O(g) A sample originally

  1. maths

    Bacl2.2H2O+KCl what the reaction?

  2. chemistry

    KCl(s) → K+(aq) + Cl‾ (aq) Solid KCl dissolves as shown in the above equation. A 6.60 g sample of KCl was dissolved in 42.3 g of water. The initial temperature of the water was 21.90°C. After the compound dissolved, the

  3. 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

  4. Chemistry

    A sample of a mixture containing only sodium chloride (NaCl) and potassium chloride (KCl) has a total mass of 4.000g. When this sample is dissolved in water and excess silver nitrate is added a white precipitate (AgCl) forms.

You can view more similar questions or ask a new question.