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What is the meaning of furnish ions?

to supply ions


What substance is acid?

Acid is a chemical substance that donates hydrogen ions when dissolved in water, leading to an increase in the concentration of protons. Examples of common acids include hydrochloric acid (HCl) and sulfuric acid (H2SO4).


How do you determine the normality of a hydrogen peroxide solution?

Normality - a unit of concentration, it focuses mainly on the H+ and OH- available in an acid-base reaction. Normality can be found by using the formula Normality =Equivalents / LitersOtherwise known as N = equiv/LEquivalent of an acid - amount of acid that can furnish 1 mol of H+ ionsEquivalent of a base - amount of base that can furnish 1 mol of OH- ionsEquivalent weight - The mass (in grams) of one equivalent of an acid or base1) Look at the subscript to figure out the equivalent acid, or how many H+ or OH- can be furnished in one mol. The subscript will help you find the equivalent weight.In this case, the formula is is H2O2.it can furnish 2 mol of H+ ions per molecule. One mol of H2O2 can furnish two mol of H+. However we only need one mol of H+. Therefore, divide by two. 1/2 mol H2O2 = 1 equivalent of H2O22) Divide by however many Liters you have.


What weight of FE3O4 will furnish 0.5430g of FE2O3?

To calculate the weight of Fe3O4 needed to furnish 0.5430g of Fe2O3, you need to consider the molar masses of Fe3O4 and Fe2O3. The molar mass of Fe3O4 is 231.535 g/mol, and of Fe2O3 is 159.69 g/mol. By using the molar ratios between Fe3O4 and Fe2O3, you can determine that 0.5430g of Fe2O3 would require 0.7799g of Fe3O4.


Why don't the electrodes of a fuel cell deteriorate the way the electrodes of a battery do?

The electrodes of a storage battery, particularly the lead - lead dioxide batteries commonly used in starting vehicles, may deteriorate because the discharge reaction requires one or both of the solid electrodes used to dissolve partially in the electrolyte, and the recharging reaction requires depositing new solid on both electrodes from the electrolyte. In order to maximize the possible output of electric current from a battery during the discharge or working phase, the electrodes have special surface characteristics that maximize their effective surface area. Both the charging and discharging phases of use of a battery of this type often decrease the effective surface area of the solid electrodes, and the recharging in particular may deposit solid on one or both of the electrodes in a shape that causes it to short to the other electrode. This does not occur in fuel cells, because the solid electrodes of a fuel cell do not dissolve during use. Instead, the electrodes serve (1) as catalysts to promote the oxidation and reduction reactions of fuels supplied to the electrodes as liquids or gases dissolved in the electrolyte and (2) to accept or furnish the electrons needed for the reactions to occur at separate locations. Furthermore fuel cells never need recharging, because the reactants consumed are replenished from outside the fuel cell itself and not regenerated within the cell, as for a storage battery.