Which statement is false regarding hydrofluoric acid (HF)? NaF is a source of HF when dissolved in water.   HF can be toxic if spilled on your skin because if it penetrates to your bones, it will react with the calcium ions to form CaF2.   The corrosive property of HF is a sign that it is a strong acid.   HF will react with glass (SiO2) to produce water.

Some chemical reactants are listed in the table below. Complete the table by filling in the oxidation state of the highlighted atom. oxidation state of highlighted atom 0 0 species FeSO4(s) VO(s) Fe₂O3(s) KMnO4(s) X 0 0

Use the Lewis structure shown to assign oxidation states of each indicated atoms. (There are two different carbon atoms, labeled C1 and C2.)     C1:   C2:

Provide Proper IUPAC names Provide Proper IUPAL name CH3 No2 (H3 OF HOCCC H2)3COH gletaric acid]

Some chemical reactants are listed in the table below. Complete the table by filling in the oxidation state of the highlighted atom. oxidation state of species highlighted atom FeO(s) Cl2(9) SiO2(9) ОН (ад)

When you have an "upset stomach", most people consume a chemical known as an antacid. Antacids contain the chemical Al(OH)3 which reacts with stomach acid (HCI) in the reaction below. This reaction, between an acid and a base, is commonly called a neutralization. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: (antacid) (stomach acid) Al(OH)3(s) + 3 HCI(aq) --> AICI3(aq) + 3 H20() 78.006 36.461 133.341 18.016 How many moles of stomach acid can be neutralized by 3.60 mol of antacid?

In an experiment, a student combines 75.0 mL of a 0.200 M iron (III) chloride solution with 125.0 mL of a 0.250 M sodium carbonate solution. Write a balanced equation for the reaction. What is the limiting reactant? What is the theoretical yield of sodium chloride (in grams)? How many grams of sodium chloride need to be produced in the experiment in order to achieve a yield of 93.75%?

A mixture contains only NaCl and Al2(SO4)3. A 2.67-g sample of the mixture is dissolved in water and enough amount of NaOH is added, producing a precipitate of Al(OH)3. The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.754 g. What is the mass percent of Al2(SO4)3 in the sample? Assume that all aluminum is precipitated as Al(OH)3.

1. If 30.4 g of Nal (MM=149.89g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of Nal in the resulting solution? 2. What volume (in L) of 1.1 M FeCl3 would be required to obtain 0.59 moles of Cl- ions?

40.00 mL of a solution of MgCl2 with a molar volume concentration of 0.933 mol/L is mixed with 100.0 mL of a solution of AlCl3 with a molar volume concentration of 0.211 mol/L.  What is the final molar volume concentration of chloride ions (Cl-) in the mixture in mol/L? Note: The density of pure water is 1.000 g/mL.