A solution containing a mixture of metal cations was treated with dilute HCl and a precipitate formed. The solution was filtered and H2S was bubbled through the acidic solution. A precipitate again formed and was filtered off. Then, the pH was raised to about 8 and H2S was again bubbled through the solution. This time, no precipitate formed. Finally, the solution was treated with a sodium carbonate solution, which resulted in formation of a precipitate. Which metal ions were definitely present, which were definitely absent, and which may or may not have been present in the original mixture? Ag+, Zn2+, Co2+, Li+, Cu2+, Ca2+, Fe2+, Sn2+, Mg2+, Hg22+ Sb3+, Hg2+, Pb2+

1. Add the periodic trend of electronegativity to your periodic table.
2. On your periodic table underline the elements that make up the 7 diatomic molecules (from chapter 6.6) and add the periodic trends of ionization energy, atomic size, and metallic character (chapter 4.8).

Please explain...

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?

a. an indicator with Ka = 10–13

b. an indicator with Ka = 10–14

c. an indicator with Ka = 10–10

d. an indicator with Ka = 10–8

e. an indicator with Ka = 10–11

An indicator HIn has Ka = 1 × 10–8. At pH = 6.0, what is the ratio HIn/In– ?

a. 1/100

b. 10/1

c. 1/1

d. 100/1

e. none of these

balance redox reaction that occurs in acidic conditions. what are coefficients for H + & Fe3+ once reaction is balanced? write it as H+=#; Fe +3 = #

Fe2+(aq)+Mn04-(aq) -> Fe3+(aq)+Mn2+(aq)

1. Ph of H3O+ of 5.7x10^3
2. Ph of a 1.5x10^-2 m for HBr

3. ph of 3.24x10^-4 m of hypochlorous acid ka2.9x10^-8

In organic chemistry, we have ortho/para activators and deactivators. Why do we not have meta activators?

Indicate the concentration of each ion present in the solution formed by mixing the following. (Assume that the volumes are additive.)

(a) 40 mL of 0.100 M HCl and 10.0 mL of 0.600 M HCl

H⁺ ________ M

Cl ^- ________ M


(b) 15.0 mL of 0.300 M Na₂SO₄ and 20.6 mL of 0.200 M KCl

Na⁺ _________ M

K⁺ __________ M

SO₄^2- __________ M

Cl ^- __________ M


(c) 3.50 g of NaCl in 40.6 mL of 0.365 M CaCl₂ solution
Na⁺ ___________ M

Ca²⁺ __________ M

Cl ^- __________ M

Calculate the hydronium ion concentration and the pH when 65.0 mL of 0.45 M NH3 is mixed with 65.0 mL of 0.45 M HCl (Ka = 5.6x10^-10).

Concentration =

pH=

In my text book it states: The relative atomic mass of an element is the average mass of an atom of the element, taking into account all its isotopes and their relative abundance, compared to one atom of carbon 12. At the same time it states that generally, the relative atomic mass is the mass of one mole of atoms of an element. So is it the mass of one moles of atoms of an element or the average mass of an atom of the element?

MATCH EACH TYPE OF CRYSTALLINE SOLID TO THE APPROPRIATE EXAMPLE: 1. ATOMIC 2.METALLIC 3.IONIC 4. NETWORK COVALENT 5.MOLECULAR

A)C (GRAPHITE) B)N2 C)Kr D)Au e)MgBr2

Distinguish linear range, dynamic range, and range.

The pH of a 0.120 M solution of a weak base is 10.97 at 25ºC. Calculate the pH of a 0.0316 M solution of this base at 25ºC.

derive BET isotherm adsorption equation step by step