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2CrO42-(aq) + 2H+ to Cr2O72-(aq) + H2O(l). Identify the reactant or product that increased or decreased when NaOH was added.
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- What is the conjugate acid of H2C6H7O5 -1aq2? What is its conjugate base?Fill in the left side of this equilibrium constant equation for the reaction of diethylmethylamine (C,H13N), a weak base, with water. Ü - K,2CrO42-(aq) + 2H+ to Cr2O72-(aq) + H2O(l). Identify the reactant or product that increased or decreased when HNO3 was added.
- Given the following information:HF (aq) ↔H+(aq) + F–(aq) Kc = 6,8 x 10–4H2C2O4 (aq) ↔ 2 H+(aq) + C2O42–(aq) Kc = 3,8 x 10–6Determine the value of Kc for the reaction: 2 HF (aq) + C2O42–(aq) ↔ F–(aq) + H2C2O4 (aq)What is the product of the following acid-base reaction:Mg(OH)2 + H3PO4→ Mg3(PO«)2 + H2O
- CO2 + H2O→H2CO3 → HCO3– +H+ → CO2– +2H This chemical reaction can produce 1) a small number of hydrogen ions 2) a large number of hydrogen ions 3) a high pH value 4) anoxiawhat is the conjugate acid of C6H5NH2?What type of product would the following reaction be most likely toproduce? Explain your reasoning.Ba(OH ) 2 (aq) + 2HCl(aq) →
- Complete the following reaction schemeThe amount of tartaric acid is responsible for the tartness of wine and controls the acidity of the wine. Tartaric acid also plays a very significant role in the overall taste, feel and color of a wine. Tartaric acid is a diprotic organic acid The chemical formula for tartaric acid is C4H6O6 and its structural formula is HO2CCH(OH)CH(OH)CO2H. A 50.00 mL sample of a white dinner wine required 21.48 mL of 0.03776 M NaOH to achieve a faint pink color. Express the acidity of the wine in terms of grams of tartaric acid, H2C4H4O6 (M. M. = 150.10) per 100 mL of wine. Assume that the two acidic hydrogens are titrated at the end point. MM H2C4H4O6 = 150.10 MM NaOH = 40.00 Below is the balanced chemical equation for this titration.What is the product and what kind of reaction is this?