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Identify the reagents necessary for the reaction:
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- A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?HgOA), H₂O/THE NaBH||| O crosoft O 3 Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) NaCl(aq) + H₂O(l) + CO₂(g) The CO₂ gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 200. mL of a 0.072 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits. W CHEMICAL REACTIONS Solving for a reactant in solution Microsoft Microsoft 6.52.210... 08 g Explanation 10 Check 280 x10 X 2 NOV 13 Ś ||| - K Jay SETMANES tv ♫ MacBook Pro DZA . E © 2022 McGraw Hill…
- Can anyone step by step （in details）explain how we get 2HNO2 from nitric acid？how does we get the equation？The pH scale for acidity is defined by pH – log10 H*| where |H*| is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of Drano is 13.3. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M (B) The pH of rain water is 5.5. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M1. Consider the titration of 25.00 mL of 0.150 M acetic acid (HC2H3O2, Ka = 1.8 × 10−5 ) (aq) with 0.175 M NaOH(aq). What is the pH of the titration solution . . . a. . . . before any NaOH is added? b. . . . after 10.00 mL of NaOH is added? c. . . . at the equivalence point? Also, what volume of NaOH is required to reach this? d. For this titration, which is the best indicator to use: phenolphthalein, bromothymol blue, or methyl orange? Justify your answer
- The average blood pH is 7.40. The blood volume in humans, on average, is 5 liters. On average bicarbonate concentration in blood is 25 mM. A vinegar jar has a label that says its acetic acid concentration is 3.0%, meaning 3.0 g of acetic acid in 100 mL vinegar. (1) How many mL of vinegar does a person have to intake in order to lower the blood pH to 7.25? (2) if ALL the bicarbonate in 5.0 L of blood is neutralized by vinegar, how many mL of vinegar will be needed? (3) When all the bicarbonate ions are neutralized to carbonic acid, what will be the resulting blood pH? Note: pKa values for carbonic acid (diprotic acid) are 6.4 and 10.3, respectively.Q7. Karl Fisher titration is used to determine moisture content of food products according to the chemical reaction below: 2H₂O + SO₂ + 12 → H₂SO4 + 2HI (i) Name the reaction that involved. (ii) Identify the FOUR major chemical components needed in the Karl Fisher reagents. (iii) Rewrite the actual chemical reaction(s) that involved during Karl Fisher titration. (iv) Outline the function of each major chemicals in the reaction stated in answer (iii).ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?
- Constants | Periodic Table These questions refer to determing unknown concentrations of acids and/or bases. Part A In a titration experiment, a solution of rubidium hydroxide (RBOH) of unknown concentration was titrated with a solution of nitric acid (HNO3) of known concentration. 15.00 mL of the unknown rubidium hydroxide (RbOH) solution required 23.21 mL of 0.1429 mol L-1 nitric acid (HNO3) solution. What is the concentration of the rubidium hydroxide (RbOH) solution? OH 9.235x10-2 mol L-1 0.2211 mol L-1 0.2322 mol L- 0.1429 mol L-1 0.2587 mol L |-1The acidity of a solution is measured by its pH. If HT| represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH = – log H+ Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 37.93% greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 4.36, determine the pH of Solution A. Report your answer to two decimal places. Solution A has pH equal to Number - (Report to the nearest 0.01)> Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) → NaCl(aq) + H₂O(1) + CO₂(g) - A The CO₂ gas produced is what makes you burp after drinking the solution. ol Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 200. mL of a 0.067 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Round your answer to 2 significant digits. ng 5.0 x10 X ? 5 Was
