H2SO4 (aq) + 2 NaHCO3 (s) -> Na2SO4 (aq) + 2 H2CO3 (l) GIVEN: - I've converted 25.0 mL to. Well H2SO3 is stronger than H2SeO3 not vice versa. H2SO3 H2SO4 H2SeO3 H2SeO4 For oxyacids, the acidity increases with increasing number of oxygen atoms; therefore, H2SO3 and H2SeO3 will be weaker than either H2SO4 or H2SeO4. But k2 is a weak acid (not ionized 100%) but is still relatively large as K2s go. SO2(g) + H2O(l) → H2SO3(l) What mass of sulfur dioxide is, rank strongest acid to weakest acid? I looked up k2 for H2SO4 and H2SeO4 and both are listed at 1.2E-2. A volume of 70.0mL of aqueous potassium hydroxide(KOH) was titrated against a standard solution of sulfuric acid (H2SO4). Thus: oxigen reacts with water more easily and thereby in higher concentration. what is the strongest acid here? Hence: the binds are less energetic. Then you compare which one has higher electronegativity will have the acidic characteristic. Answer. Ka1= 1,23*10^(-2) Ka2= 6,6*10^(-8) Results attached are: a) [H2SO3]= 1,04x10-4 M, [SO32-]=1,3x10-4 M, [HSO3-]= 0,05 M but i keep getting different. Still have questions? Which is the stronger acid H2SeO4 or H2SeO3? Se is slightly larger but both have about the same electronegativity. H2SO3 The fact it's in a lower period in that group means that it's more reactive than sulphur. Therefore the binds are less ' strong' . Well, in basics, its position is closer to the bottom of the periodic table in the same group. Lets see which one is stronger. As you see they both have same oxidation numbers/Oxygen atoms number, then you will focus on the central atoms which are S … What was the molarity of the solution if 19.2mL of 1.50M H2SO4 was needed? H2SO3 + H2O --- H3O + SO I am Not sure if its is tri/mono/diprotic, Elemental sulfur can be converted to sulfur dioxide by combustion in air. Write the acid-dissociation reaction of nitrous acid (HNO2) and its acidity constant expression. 3 4 5. Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). Atoms that are larger tend to have larger acid strengths and those with increasing electronegativity of the central atom tend to be less acidic. And I hope you don't need anything more in depth because my chemistry days are long ago. which makes you more jittery coffee or tea? The strong bases are listed at the bottom right of the table and get weaker as we move to the top of the table. 1. If so, look them up. www.chemistryconcept.com H2SeO4 stronger. Acid with values less than one are considered weak. The equation is, Are these correct? The ionization constants for sulfurous acid are Ka1 = 1.4 x 10^-2 and Ka2 = 6.3 x 10^-8 so I'm trying to find Na, SO3 2-, HSO3-, H2SO3, Calculate the concentrations of H2SO3, H3O+, HSO3-, and SO32- in a 0.025 M H2SO3(aq) solution, Care must be taken when diluting sulfuric acid with water, because the dilution process is highly exothermic: H2SO4(l) "arrow" H2SO4(aq) + heat a) Find the ÄHo for diluting 1.00 mol of H2SO4(l) (d = 1.83 g/mL) to 1 L of 1.00 M, A beaker containing 25.0 mL of 0.360 M H2SO4 spills on the counter. Consider the following equilibrium system: N2(g)+2O2(g) ⇄ 2NO2(g); ? I went to a Thanksgiving dinner with over 100 guests. Therefore: H2SeO3 is more acidic than H2SO3, Well H2SO3 is stronger than H2SeO3 not vice versa. 3. ? We have a problem determining which is 14,532 results rank strongest acid to weakest acid H3CNH2 CH3C (triple bond) CH CH2=CHCH3 H20 CH4 i tried to rank them using the Pka values but I couldn't find the pKa value of the alkyne and I thought the, Calculate pH and concentration of H2SO3, H2SO3- and SO32- in NaHSO3 c=0,05M. Thats the basics of it. Wiki User Answered . Strong acids are listed at the top left hand corner of the table and have Ka values >1 2. How many people does it take to operate a mass spectrometer / spectrometry machine? The equation is, net ionic equation to show that sulfurous acid, H2SO3, behaves as an acid in water. Asked by Wiki User. In this case, S has higher electronegativity than Se, so H2SO3 is a stronger acid than H2SeO3. How does an incomplete reaction occur in steam distillation and what does it have to do with equilibrium. H2SeO4 We have a problem determining which is the stronger of H2SO4 or H2SeO4. 2011-11-28 23:34:23 2011-11-28 23:34:23. 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Both acids are strong acids; therefore, their first ionization is 100% so k1 will not be listed. Top Answer. We have a problem determining which is the stronger of H2SO4 or H2SeO4. Atoms that are larger tend to have larger acid strengths and those with increasing electronegativity of the central atom tend to be less acidic. Now, because it's in the same group, it reacts in a similar way with the same things. Join Yahoo Answers and get 100 points today. You can view more similar questions or ask a new question. Therefore it attracts oxygen's electrons more strongly and weakens the O-H bond to a greater extent, enabling H+ to be released more easily. NH3 ,H2SO4, CH3OH, CH3COOH CH3COOH > H2SO4> CH3OH >NH3 Rank the following species in order of. Calculate the concentrations of all species in a 0.810 M Na2SO3 (sodium sulfite) solution. For the formation of ammonia, N2(g) + 3H2(g) ⇌ 2NH3(g). As you see they both have same oxidation numbers/Oxygen atoms number, then you will focus on the central atoms which are S and Se. A volume of 40.0mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). The chief was seen coughing and not wearing a mask. For oxyacids, the acidity increases with increasing number of oxygen atoms; therefore, H2SO3 and H2SeO3 will be weaker than either H2SO4 or H2SeO4. I got this answer but do not know if it is correct. How much baking soda, NaHCO3, will be needed to neutralize the acid? Get your answers by asking now. The fight is between HNO3 and H2SO4 for the kingdom of acids. H2SeO3 Explain your reasons of ordering them as you do. The conjugate base HSO3-/SO3 2- is more stable than the conjugate base HSeO3-/SeO3 2-.Because selenium is larger than sulfur, its … Se is slightly larger but both … What was the molarity of the KOH solution if 21.7mL of 1.50 M H2SO4 was needed? 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