Sulfuric acid molar mass

The total aerosol mass during the variation of total ammonia in the system is also shown in Figure 10.17. One would expect that an increase of the availability of NH3, an aerosol precursor, would result in a monotonic increase of the total aerosol mass. This is not the case for at least the ammonia-poor conditions (ammonia/sulfuric acid molar ratio less than 1). The increase of NH3 in this range results in a reduction of the H2S04(aq) and the accompanying water. The overall aerosol mass decreases mainly because of the loss of water, reaching a minimum for an ammonia concentration of 1.8 pg m-3. Further increases of ammonia result in increases of the overall aerosol mass. This nonlinear response of the aerosol mass to changes in the concentration of an aerosol precursor is encountered often in atmospheric aerosol thermodynamics. 

The conclusion that all low molar mass lignins are hemilignins is, however, an oversimplification since it has been shown that, on heating an aqueous solution of glycolignin sulfonic acid acidified with hydrochloric acid or sulfur dioxide and bisulfite, a monomeric sulfonated hydrolysis product is formed (2). 

Self-Test 15.2A Concentrated sulfuric acid is 98.0% by mass H2S04. Calculate its molar concentration, given that its density is 1.84 g-mL 1. 

From the chemical equation for the reaction and using the relative formula masses together with the molar volume of a gas it is possible to predict the amounts of magnesium sulfate and hydrogen that arc produced when 24gof magnesium is reacted with excess sulfuric acid. 

Sulfuric acid compositions are expressed in mass%. For this reason, acidmaking calculations are more easily done with mass (rather than molar) balances. 

A method for the controlled emulsion polymerization of chloroprene using dithiocarbamic esters as sulfur-based chain transfer agents is described. The method provides industrially relevant molar masses with Mn s> 50,000 daltons with good yields in acceptable times. It was further determined that when pKa values for the dithiocarbamic acid precursors were less than 12, the thioester was ineffective as a regulator. 

A 0.50-molar aqueous solution of sulfuric acid flows into a process unit at a rate of 1.25 m /min. The specific gravity of the solution is 1.03. Calculate (1) the mass concentration of H2SO4 in kg/m, (2) the mass flow rate of H 2S04 in kg/s, and (3) the mass fraction of HjSO,. 

Suppose 150 mL of a 10.00% by mass solution of sodium chloride (density = 1.0726 g cm ) is acidified with sulfuric acid and then treated with an excess of Mn02(s). Under these conditions, all the chlorine is liberated as Cl2(g). The chlorine is collected without loss and reacts with excess H2(g) to form HCl(g). The HCl(g) is dissolved in enough water to make 250 mL of solution. Compute the molarity of this solution. 

As we mentioned before, we can see that the molar ratio between zinc and hydrogen is 1 1. This means that 1 mole of zinc would react with an excess of sulfuric acid to produce 1 mole of hydrogen gas. Thus, 0.02 moles of zinc are required to produce 0.02 moles of hydrogen gas. Now that we know how many moles of zinc we need (0.02 moles), we can easily convert this to grams by multiplying by the molar mass of zinc 65.4 g/mole), which we find on the periodic table. 

A sample of commercial sulfuric acid is 96.4% H2SO4 by mass, and its specific gravity is 1.84. Calculate the molarity of this sulfuric acid solution. 

What are the molarity and normality of a sulfuric acid solution that is 19.6% H2SO4 by mass The density of the solution is 1.14 g/mL. 

More than 40 million tons of sulfuric acid are produced annually worldwide. The contact process is used for the commercial production of most sulfuric acid. The solution sold commercially as concentrated sulfuric acid is 96-98% H2SO4 hy mass and is about f8 molar H2SO4. 

What volume of hydrogen gas is produced if 2.16 g of zinc metal are consumed with sulfuric acid The hydrogen gas is measured at 748 mmHg and 22°C. The molar mass of zinc is 65.4 g. The balanced equation is... 

Problem Is How many milliliters of 0.500 M sulfuric acid, H2SO4(aq), are needed to just completely react with 12.0 g of sodium hydroxide, NaOH The molar mass of NaOH is 40.0 g, and the balanced equation for the reaction is... 

Calculate the molality of a sulfuric acid solution containing 24.4 g of sulfuric acid in 198 g of water. The molar mass of sulfuric acid is 98.08 g. 

Answer From the known molar mass of sulfuric acid, we can calculate the molality in two steps. First we need to find the number of grams of sulfuric acid dissolved in 1000 g (1 kg) of water. Next we must convert the number of grams into the number of moles. Combiiung these two steps we write... 

The concentrated sulfuric acid we use in the laboratory is 98.0 percent H2SO4 by mass. Calculate the molality and molarity of the acid solution. The density of the solution is 1.83 g/mL. 

Calculate the molar mass of sulfur dioxide, a gas produced when sulfur-containing fuels are burned. Unless "scrubbed" from the exhaust, sulfur dioxide can react with moisture in the atmosphere to produce acid rain. 

Another concentration measure sometimes encountered is normality (symbolized by N). Normality is defined as the number ot equivalents per liter of solution, where the definition of an equivalent depends on the reaction taking place in the solution. For an acid-base reaction, the equivalent is the mass of acid or base that can furnish or accept exactly 1 mole of protons (H ions). In Table 11.2 note, for example, that the equivalent mass of sulfuric acid is the molar mass divided by 2, since each mole of H2SO4 can furnish 2 moles of protons. The equivalent mass of calcium hydroxide is also half the molar mass, since each mole of Ca(OH)2 contains 2 moles of OH ions that can react with 2 moles of protons. The equivalent is defined so that 1 equivalent of acid will react with exactly 1 equivalent of base. 

The first school began with Venczel s dissertation in Zurich in 196190 on the transport of ferric ion to an electrode evolving hydrogen gas from one molar sulfuric acid. Venczel found that mass transfer increased rapidly with the onset of gas evolution. Ibl and Venczel26 reported mass transfer at gas-evolving electrodes as Nemst boundary layer thicknesses that are functions of gas evolution rate... 

A case in point is a study made by Ross (J ) on the dissolution of iron in 0.5 molar sulfuric acid in the presence of thiourea at 40° C. The results of this study, which was conducted as a function of the flow rate, are shown in Fig.9. It appears that the uninhibited dissolution of iron follows expected mass transfer behavior both in the laminar and turbulent regions. However, at two inhibitor concentrations marked deviations from the expected mass transfer behavior are observed. Ross attempted to explain these results on the basis that different inhibitor concentrations affect the anodic and cathodic polarization in different ways, taking also into consideration that at small... 

Table 3.1 summarises the water solutions of sulfuric acid with concentrations expressed in mass percent (wt%), density (kg L ), molarity (mol L ) and temperature eoeffieient of density [1]. The range of acid concentrations used in lead—aeid batteries is also marked in the table. If acid solutions of higher or lower concentrations than the battery operation range (battery aeid window) are used, this would lead to a decline in performance parameters of the batteries. 

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